What volume of hydrogen gas is produced at STP when 6.5 g of zinc react with excess dilute Sulphuric acid?

3.25g of zinc was added to 50cm^3 of a 4.0 molar dm^-3 HCl. When the reaction was completed the temperature rose by 28 degrees celcius. (a) Is the reaction exothermic or endothermic? (b)All the zinc dissolve in this reaction. How many moles of zinc
Very hot zinc will react with steam to form zinc oxide and hydrogen. What volume of steam would be necessary in order to use up 20.0 g of zinc completely? What volume of hydrogen would be produced in this case? I NEED HELP WITH THIS!!..PLEASE = )
Zn+ 2HCl -> ZnCL2+h2 what volume of hydrogen at stp is produced when 2.5 of zinc react with an excess of hydrochloric acid
A 0.052g sample of aluminium reacts with excess 6M HCL. A 48.3mL volume of hydrogen gas was collected over water at 22C and the pressure of the hydrogen gas was 751mmHg.calculate the aluminum percent purity in the sample. What volume of hydrogen gas at STP
10. If the calcium oxide were obtained by the heating of calcium hydroxide, how much hydroxide would be needed to obtain the 15.0 g? 11. If the 15.0 g of calcium oxide in the above problems were allowed to react with water, what amount of calcium hydroxide
6.5g of zinc was reacted with excess HCL.calculate the volume of dry hydrogen gas. my work zn+2HCL-zncl2 + H2
Mg + 2HCl ----> MgCl2 + H2 What volume of hydrogen at STP is produced from the reaction of 50.0g of Mg and the equivalent if 75g of HCl? 1. What is the limiting reagent? 2. What is the volume of hydrogen produced? 3. How much is in excess?
When zinc metal is reacted with hydrochloric acid, zinc chloride and hydrogen gas are produced. If 25ml of 0.2M HCl and 0.3g of zinc metal is used: a. how many M of zinc chloride will be produced? b. how many M of zinc chloride will be produced if 0.5M of
the purity of zinc is to be determined by measuring the amount of hydrogen formed when a weighed sample of zinc reacts with an excess of HCL acid.the sample weighs 0.198 grams. what amount of hydrogen gas at STP will be obtained if the zinc is 100% pure?
A sample of zinc metal reacts completly with an excess of hydrochloric acid: Zn(s) + 2HCl(aq) --> ZnCl2(aq) + H2(g) The hydrogen gas produced is collected over water at 25.0 °C. The volume of the gas is 78.0 L & the pressure is 0.980 atm. Calculate the
An excess of a divalent metal M was dissolved in a limited volume of hydrochloric acid. If 576cm^3 of hydrogen were liberated at S.t.p , what was the mass of metal that produced this volume of hydrogen.(M=24,H=1, molar volume of a gas at s.t.p =22.4dm^3.
Suppose that 50.0 cm3 of 2.00 M hydrochloric acid are added to 4.00 grams of zinc metal. What it the limiting reagent? How many grams of zinc are actually consumed? What is the concentration of the hydrochloric acid solution after the reaction has
Calculate the number of moles of calcium chloride Cacl2 that can be obtained from 25g of limestone CaCo3 in the presence of excess hydrogen chloride
16.2g of magnesium reacts exactly with 25.3g of fluorine to produce magnesium fluoride, the only product. How many grams of magnesium fluoride could be produced from the reaction of 10.5g of magnesium with excess fluorine. This is simple if you use
22.0 grams of zinc reacted with 95.0 mL of 0.5 Molarity HCl. What volume of hydrogen gas would be produced at 22 degrees C and 745 torr?
Zinc metal reacts with hydrochloric acid to produce hydrogen gas according to the equation below. What volume of hydrogen at STP is released when 15.1 grams of zinc react at STP? Zn(s) + 2HCl(aq) �¨ ZnCl2(aq) + H2(g)
Hydrogen gas is produced when zinc reacts with hydrochloric acid. if the actual yeild of this reaction is 85%, how many grams of zinc are needed to produce 112L of H2 at STP?
472 mL of H2 gas was collected over water when 1.256 g of Zn reacted with excess HCl. The atmospheric pressure during the experiment was 754 mm Hg and the temperature was 26 degrees C. A. Write the balanced chemical equation (I have this) Zn + HCl --->
What volume of hydrogen would be produced by the reaction of 2.00g of Mg with an excess of hydrochloric acid at STP. Using this equation Mg+HCl
what volume of hydrogen gas, measured at STP, will be produced when 16.0g of magnesium reacts completely with an excess of hydrochloric acid
10.5g of zinc trioxocarbonate(iv) were heated very stronglu to a constant mass and the residue treated with excess Hcl.calculate the mass of zinc chloride
12.5g of zinc trioxocarbonate were heated very strongly to a constant mass and the residue treated with excess hydrochloric acid .calculate the mass of zinc chloride that would be obtained ?
10.5g of Zinc trioxocarbonate (iv),were heated very strongly to a constant mass and the residue treated with excess hydrochloric acid. Calculate the mass of Zinc chloride that would be obtained
2Na + 2H2O = 2NaOH + H2 Calculat the moles and volume of hydrogen produced when 0.2 moles of sodium reacts with excess water.
Write balanced net ionic equAtions. D) zinc chloride and excess ammonia E) cupric phosphate and lots of ammonia A) ammonia and excess zinc sulfate
I am completing my lab and cannot figure this out. I need someone to go over it and make sure I am right because I can't figure out why my empirical formula does not match the molecular formula. #7 is the one I am really having a problem with, but here is
Magnesium metal reacts with hydrochloric acid to produce hydrogen gas H2 Mg + 2HCl ----> MgCl + H2 Calculate the volume (in liters) of hydrogen produced at 33 degrees C and 665 mmHg from 0.0840 mol Mg and excess HCl P= .875 atm V= ? n= .0840 mol R= 0.0821
Consider the following reaction: 2H2 (g) + O2 (g)  2H2O (l) ΔH = -572 kJ a. How much heat is evolved for the production of 1.00 mol H2O (l)? b. How much heat is evolved when 4.03 g hydrogen is reacted with excess oxygen? c. How much heat is evolved
What mass of hydrogen gas is produced when a 7.43 g chunk of zinc dissolves in 500.0 mL of 1.200M HCl?
Small quantities of hydrogen gas can be prepared in the laboratory by the addition of aqueous hydrochloric acid to metallic zinc. Zn(s)+2HCl(aq) -> ZnCl2(aq)+ H2(g) Typically, the hydrogen gas is bubbled through water for collection and becomes saturated
Calculate the volume of hydrogen produced by the electrolysis of 54.0 mL of water at 27.°C and 1.3 atm, using the ideal gas approximation.
A student carried out an experiment to find the rate of decomposition of hydrogen peroxide into water and oxygen gas. The student used 100 cm3 of a 1M solution of hydrogen peroxide at 25°C and 1 atm pressure. 1 g of powdered MnO2 as a catalyst was added
2Na(s) + 2HCl (aq) -> 2NaCl (aq) + H2 (g) 1. IF 2.5G OF SODIUM REACTS WITH AN EXCESS OF HYDROCHLORIC ACID, WHAT VOLUME OF HYDROGEN WILL BE PRODUCED? My working: Na H2 mass-2.5 0.109 mr-23 2 moles-0.109 0.543 volume 0.109 X 24000 = 2608.696cm3 Is that
Phosphoric acid reacts with zinc to produce hydrogen gas and zinc phosphate. How many grams of acid are required to produce 5.3 liters of hydrogen at 743mmHg and 27.0 degrees Celsius
A mixture of chromium and zinc weighing .362 g was reacted with an excess of hydrochloric acid. After all the metals in the mixture reacted 225 mL of dry hydrogen gas was collected at 27 C and 750 torr. Determine the mass percent Zn in the metal sample.
Solid zinc and aqueous hydrogen sulfate reacts to produce hydrogen gas and aqueous zinc sulfate Is this the right answer Z(aq)+HS equals H(G) ZS? if not can u please correct me
Given the balanced equation N2(g)+3H2(g)==>2NH3 Calculate: a)the volume H2 that reacts with 12L of N2 b)the volume of NH3 produced Iron 4L ofN2 c)the volume of N2 and H2 to produced 60L of NH3 Assume that all volume measurements are made under identical
If 26.5 mL of 0.222 M HCl reacts with excess Mg, how many mL of hydrogen gas are produced at STP?
1. If 29.0 L of methane, CH4, undergoes complete combustion at 0.961 atm and 140°C, how many liters of each product would be present at the same temperature and pressure? My answer: (0.961 atm)(29.0 L) (413k) all divided by (413)(0.961 atm)=29.0 L CO2
Some hydrogen is collected over water at 10 degrees C and 105.5 kPa pressure. The total volume of the sample was 1.93 L. Calculate the volume of the hydrogen or reacted to STP.
If 20 grams of zinc reacts with hydrochloric acid, how much zinc chloride is produced?
Using the activity series, write a balanced chemical equation for the following reactions: 1. iron metal is added to a solution of copper (II) nitrate 2. zinc metal is added to a solution of magnesium sulfate 3. hydrobromic acid is added to tin metal 4.
How many grams of solid zinc metal will completely react with 100.0 mL of 0.0525 M HCl, if zinc chloride and hydrogen gas are the only products?
The products of the reaction between zinc and sulfruric acid are zinc sulfate, hydrogen sulfide, and water. Balance the equation using the electron-transfer method
Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (a) Nickel metal is added to a solution of copper (II) nitrate; (b) a solution of zinc nitrate is added to a
a chemist reacts 8.85g or iron with an excess oh hydrogen chloride to form hydrogen gas and iron(II)chloride.calculate the theoretical yield and the percentage yield of hydrogen if 0.27g H2 are collected
Suppose that 0.205 g of a mixture containing Na2SO4 and K2SO4 is dissolved in water. An excess of BaCl2 is added and a precipitate of 0.298 g of BaSO4 is produced. Calculate the percent by mass of Na2SO4 and K2SO4 in the original mixture.
When 1.38 g of magnesium is added to 25 mL of 2.0 M hydrochloric acid, hydrogen gas is released according to the equation below: Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g) Calculate the volume of the gas formed at STP
Show how you would calculate the % yield of hydrogen if 40.0 grams of magnesium react with an excess of nitric acid producing 1.70 grams of hydrogen gas. Mg + 2 HNO3 ---> Mg(NO3)2 + H2
1. When 20cm^3 of a gaseous Allene burns in an excess of oxygen, 60cm^3 of carbon dioxide are formed. Both volumes are measures at r.t.p. What is the formula of alkene? Is it C3H6 or C6H12 and why? 2. A student investigate the reaction of vegetable oil
A mixture contained zinc sulfide, ZnS, and lead sulfide, PbS. A sample of the mixture weighing 6.12 g was reacted with an excess of hydrochloric acid. The reactions are given below. ZnS(s) + 2 HCl(aq) → ZnCl2(aq) + H2S(g) PbS(s) + 2 HCl(aq) → PbCl2(aq)
Calculate the volume of amonia gas is produced at STP when 140g of nitrogen gas reacts with 30g of hydrogen gas (Atomic mass N=14u,H=1u)
The attendances at a high school basketball games seems to be affected by the success of the team. Look at the table and decide what function would represent the data shown. attendance 150 200 250 300 350 wins 2 4 6 8 10 a) a=2(3)^g b) a=-25g+100 c)
How many grams of hydrogen gas be produced from the reaction of 3 g of magnesium with 4 g of hydrochloric acid. identify the limiting in excess reactants. Please help btw that's the exact question.
The first step in the process used to recover zinc metal from zinc sulfide ore is the reaction of zinc sulfide with oxygen gas to produce zinc oxide and sulfur dioxide. 2 ZnS(s) + 3 O2(g) → 2 ZnO(s) + 2 SO2(g) When the external pressure is 142700 Pa and
What volume is produced when 10g of propyne is burnt in excess oxygen at S. T P
If 26.5 mL of 0.222 M HCl reacts with excess Mg, how many mL of hydrogen gas are produced at STP? Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) Group of answer choices 65.9 mL 26.5 mL 132 mL 22 400 mL 165 mL
Determine the mass of zinc sulphide, ZnS, produced when 6.2g of zinc and 4.5g of sulphur are reacted. Equation given: Zn + S8 >> ZnS Balanced equation: 8Zn + S8 >> 8ZnS nZn= 6.2 g/ (65.39 g/mol) = 0.095 mol nS8= 4.5 g/(256.48 g/mol) = 0.018 mol nS8 = 0.095
According to the following reaction, how many grams of zinc hydroxide will be formed upon the complete reaction of 29.8 grams of water with excess zinc oxide? ZnO (s) + H2O (l) Zn(OH)2 (aq)
If an excess of nitrogen gas reacts with 25.0 L of hydrogen gas, according to the reaction below, how many L of ammonia will be produced? N2(g) + 3H2(g) ---> 2NH3(g)
Excess lead (II) nitrate solution is added to 1.30 g of zinc powder and the mixture is stirred. When the reaction is finished the lead formed is filtered, dried and weighted. It has a mass of 3.31 g. What is the percentage yield of the lead? Pb(NO3)2 + Zn
1) 30cm3 of methane and ethane mixed with 100cm3 of O2 at RTP. Explosion occurs, on cooling 61.5cm3 remained. Find the percentage by volume of each gas in the mixture 2)32cm3 of a mix of CO2, CH4 and H2 mix with 50cm3 of O2 and exploded after cooling to
What volume of steam is produced when 10g of propyne is burnt in excess oxygen at STP
If 6.5g of zinc react with 5.0 of HCl according to the following reactant, which substance is the limiting reactant? How many grams of the reactant remain unreacted? How many grams of hydrogen would be produced?
Thank you for your reply. The Zn in grams 1.80= .028 moles Zn and Cl in grams 0.90= .025 moles Cl The question was: What is the EXPERIMENTAL empirical formula of zinc chloride? Determine the simplest whole number ratio of moles of zinc used, to moles of
Zinc is often used to calibrate calorimeters because it undergoes a very sharp phase transition from the solid to the liquid at 419.5°C. Calculate the enthalpy change when 5 g of zinc metal is heated from 100°C to the point where the entire sample is
Gold can be recovered from sea water by re- acting the water with zinc, which is refined from zinc oxide. 2 ZnO(s) + C(s) −→ 2 Zn(s) + CO2(g) 2 Au3+(aq) + 3 Zn(s) −→3 Zn2+(aq) + 2 Au(s) The zinc displaces the gold in the water. What mass of gold
Oxygen gas and water are produced by the decomposition of hydrogen peroxide. If 10.0 mol of H2O2 decomposes, what volume of oxygen will be produced? Assume the density of oxygen is 1.429g/L. 2H2O2= 2H2O+O2
what volume of hcl solution of density 1.2g/cm3 and containing 36.5% by weight hcl, must be allowed to react with zinc in order to liberate 4g of hydrogen I know this calculate this part, but I do not get the answer 333.3ml 1.2g/ml x 1000 x 0.365/36.5 =
Calculate the mass of water produced when 1.47 g of butane reacts with excess oxygen.
Calculate the mass of water produced when 6.51 g of butane reacts with excess oxygen.
Calculate the mass of water produced when 3.64 g of butane reacts with excess oxygen.
Gold can be recovered from sea water by reacting the water with zinc, which is refined from zinc oxide. The zinc displaces the gold in the water. What mass of gold can be recovered if 2.00g of ZnO and an excess of sea water are available? 2ZnO + C -> 2Zn +
What volume of hydrogen at STP is produced from the reaction of 50.0 g of Mg and the equivalent of 75g of HCl?
Is this correct? What is the experimental empirical formula of zinc chloride? Determine the simplest whole number ratio of moles of zinc used, to moles of chlorine reacted in the zinc chloride that was produced..028 moles of Zinc .025 moles of Cl .025
What volume of hydrogen gas measured at 27celcius and 723 torr may be prepared by the reaction of 8.88 grams of gallium with an excess of hydrochloric acid? Ga+ HCl ==> GaCl3 + H2
Ammonia, NH3, is widely used as a fertilizer and in many household cleaners. How many moles of ammonia are produced when 6 mol of hydrogen gas react with an excess of nitrogen gas?
I am given a question where I have to state which combination of electrodes will result in the greatest voltage and which will result in the lowest voltage. The metals given are Zinc, Copper, Silver and Hydrogen I think that silver and copper would give
Based on the following chemical equation answer the question below show all your calculation The balanced chemical reaction of iodine with hydrogen sulfide h2s(g)+i2(s)-----2HI(g) + S(s) (a) Based on the above chemically balanced equation, how many grams
what volume of hydrogen will be produced if 100cm3 of ammonia is completely decomposed at constant temperature and pressure.
10.2 g of Pb(NO3)2 are dissolved in 100 mL of water, and added to 250.0 mL of a 0.250 M solution of KI. Determine the mass in grams of Pbl2 produced, and find the number of moles of the excess reagent. PLZ explain
Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g) If 1.0g of Mg is reacted with 10.0mL of 6.0M HCl, what volume of hydrogen gas will be produced at 298K & 1atm?
the reaction of 7.10g carbon with excess O2 yields 12.25g of CO2. what is the percent yield of this reaction? I have tried everything and looked through all of my notes and nothing is working for stiochiometry
(I corrected it ) 1. Sodium and water react according to the following equation. If 31.5g of sodium are added to excess water, how many liters of hydrogen gas are formed at STP? 2Na+2H2O—>2NaOH+H2 My work: For #1 Na would have 2 moles and H would have 1?
what volume of carbon dioxide is produced from the reaction of 12.8 liters of oxygen with excess carbon disulfide?
Hydrogen gas is produced when zinc reacts with sulfuric acid: Zn(s)+H_2SO_4(aq)---ZnSO_4(aq)+H_2(g) If 160 mL of wet H_2 is collected over water at 24 Celsius and a barometric pressure of 739 torr, how many grams of Zn have been consumed? (The vapor
What volume (mL) of sulfur dioxide can be produced by the complete reaction of 3.82 g of calcium sulfite with excess HCl, when the final SO2 pressure is 827 torr at 44 degrees celsius?
A flexible container at an initial volume of 5.12 L contains 7.51 mol of gas. More gas is then added to the container until it reaches a final volume of 18.3 L. Assuming the pressure and temperature of the gas remain constant, calculate the number of moles
Calculate the mass of water produced when 3.09g of butane reacts with excess oxygen. 2C4H10 + 13O2-->10H2O + 8CO2 Help.
Calculate the mass of hydrogen formed when 25 grams of aluminum reacts with excess hydrochloric acid. (AM of Al= 26.9g/mol) 2Al + 6HCl ----> Al2Cl6 + 3H2
Calculate the final concentration of a. 4.0 L of a 4.0 M HNO3 solution is added to water so that the final volume is 8.0L b. Water is added to 0.35L of a 6.0M KOH solution to make 2.0L of a diluted KOH solution. c.A 20.0 mL sample of 8.0% (m/v)NaOH is
Hydrogen gas can produced by the reaction between metallic aluminum and aqueous hydrochloric acid 2Al+6HCl----2AlCl3+3H2 Hydrogen gas produced by this reaction is typically collected via water displacement, during which time the hydrogen gas becomes
I need the oxidation half reactions, reduction half reactions, and net ionic equations for the following reactions: 1)magnesium +0.1M zinc sulfate 2)copper+0.1M zinc sulfate 3)zinc+0.1M copper(II)sulfate 4)zinc+3M HCl 5)copper+3M HCl 6)0.1M potassium
Magnesium metal reacts with hydrochloric acid to form magnesium chloride and hydrogen gas. Suppose we react an excess of magnesium metal with 13.2 mL of a 3.00 M solution of hydrochloric acid and collect all of the hydrogen in a balloon at 25oC and 1.00
metal hydrides react with water to form hydrogen gas and the metal hydroxide. How do you calculate the mass of hydrogen gas that can be prepared from 3.78 g of SrH2 and 3.5 g of H2O? a) how many moles of H2 can be produced from given mass of SrH2? b) How
6 mol sample of Cu2S is roasted in excess O2 to yield Cu metal and SO2. Calculate the mass of Cu metal produced
Why is it easier to remove excess acetic acid from isopentyl acetate than excess isopentyl alcohol? Sodium Bicarbonate is added but the question doesn't say anything about it.
24g of magnesium reacts dilute hydrochloric acid calculate the volume of hydrogen gas evoled at s.t.p [Mg = 24, molar volume of a gas at s.t.p = 22.4dm
Use the equation below to answer the following questions. Al + H2SO4 ==> Al2(SO4)3 + H2 A. If 8.15 moles of aluminum are reacted, how many moles of hydrogen will be produced? B. If 44.7 g of hydrogen sulfate is reacted, what mass of aluminum sulfate is
Zinc iodide is dissolved in 2.5 L of water to make a solution. 1.00 L of this solution is then diluted to make 12.0 L of a 0.50 M solution. What mass of zinc was added to make the original solution?

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Calculate the % empty space in 1 mole of water at 25 degree C (d=0.9971g/ml). The volume of a water molecule can be taken as the sum of the volumes of the 2 hydrogen molecules and the oxygen atom. Use the single bonded covalent radii of 37pm for hydrogen
Use the following information to identify element A and compound B, then answer questions a and b. An empty glass container has a mass of 658.572 g. It has a mass of 659.452 g after it has been filled with nitrogen gas at a pressure of 790. torr and a
How do you calculate the % empty sapce in 100mL of air. Using Avogadro's number(6.02x10^23) and the average volume of O2 and N2(3.8x10^-24 cm3/molecule). I think you can use the ideal gas law but am not really sure how to do it. I also have a similar
1) Empirical formula for zinc chloride (show calculation) 2) Balanced chemical equation for the formation of zinc chloride from zinc and HCL
Write the balanced net ionic equation for the following? a) Copper metal and zinc ion b) zinc and cupric ion c) Copper metal and hydrogen ion d) zinc metal and hydrogen ion e) iron metal and hydrogen ion f) Chlorine (Cl2) and bromide ion (Br-) g) Chlorine
Hydrogen is generated by passing hot steam over iron, which oxidizes to form Fe3O4 in the following equation. 3Fe(s) + 4H2O(g) -> 4H2(g) + Fe3O4(s) Atomic Mass Fe = 55.85 g/mol Molar Mass Fe3O4 = 231.55 g/mol Molar Mass H2 = 2.02 g/mol Molar Mass H2O =
How many moles of oxygen are produced from the decomposition of 3.4g of hydrogen peroxide? How many molecules of O2 are produced?
i am working on a practice worksheet and need help with a few i can not understand. please and thank you. I have to post them separately sorry 49.how many grams of water are needed to completely hydrolyze 30.8 g of the ester? A.0.416 g B.30.8 g C.11.3 g
pyrite, FeS2 reactswhen it is heated strongly in the air according to the equation 4 FeS2(s) + 11 O2 rightarrow 2 Fe2O3(s) + 8 SO2(g) What volume of sulfir dioxide ( measured at room temprature and pressure) would be produced by heating 100g of pyrite in
Describe how you would obtain pure crystals of Sodium chloride from a muxture of solid sodium chloride and solid zinc carbonate Step1 Step 2 Step 3 1. Add HCl to react with the carbonate. The products are zinc chloride, CO2, and water. The CO2 leaves as a
What would be made if hydrogen sulphide gas was bubbled through a solution of zinc nitrate
A metal is made from copper,zinc, and lead in the ratio 13:6:1.The mass of zinc is 90kg. Calculate the mass of the metal
Nh3+Cuo=N2+Cu+H2O, 18.1g of nh3 and 90.4g of CuO made to react. (a). Determine the limiting reagent. (b). Which reactant is in excess? (c). Calculate the mass of Cu that forms. (d). Calculate the volume in liter of n2 that form at STP.
brass is a subtitutional alloy consisting of a solution of copper and zinc. a particulae sample of red brass consisting of 80% copper and 20% zinc by mass has a density of 8750kg/m^3. a. what is the molality of zinc in the solid solution and B. what is the
Consider the reaction 3Fe(s) + 4H2O(g) �¨ 4H2(g) + Fe3O4(s). If the volume of the container is reduced, 1. more Fe(s) is produced. 2. no change occurs. 3. more H2O(g) is produced. 4. more H2(g) is produced. 5. the equilibrium constant increases.
(1)Aluminum reacts with oxygen to produce aluminum oxide according to the following reaction: 4Al(s) + 3O2(g) → 2Al2O3(s) Calculate the moles of Al2O3 produced when the reaction is performed with 31.06 g of each reactant. (2)Nitrogen dioxide reacts with
a solution is made by combining 10.0 ml of 17.5 M acetic acid with 5.54 g of sodium acetate and diluting to a total volume of 1.50 L. a)calculate the pH of the solution. b) how many grams and milliliters of 14.6 M potassium hydroxide needs to be added so
I have a few question for my review. 1) How would you prepare 30.0 ml of 0.600M HNO3 From a stock solution of 4.00M HNO3? What volume in ML of the 4.00 M HNo3 will you need? 2) if a 83.5 & was repoarted for a reaction that could have produced 12.1 g of
What is the approximate volume of 0.095 M HCl needed to neutralize 0.25g of sodium carbonate. Hint: Write a balanced equation first.
ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation. N2+3H2g----- > 2NH3g. what is the maximum mass that can be produced from a mixture of 2.00×10³gN and 8.00×10⁴H2?
Methanol CH3Oh can be produced by reacting carbon monoxide and hydrogen gas in the presence of a catalyst. If 75.00 grams of carbon monoxide reacts with 106.3 grams of hydrogen, 68.40 grams of methanol are produced. What is the percent yield of methanol?
If 6.57 g of iron are reacted with an excess of hydrochloric acid, HCI, then hydrogen gas and14.63 g of iron (III) chloride are obtained. calculate the theoretical yeild and percent of yeild of FeCl3.
When hydrochloric acid reacts with magnesium metal, hydrogen gas and aqueous magnesium chloride are produced. What volume of 5.0 M HCI is required to react completely with 3.00 g of magnesium?
When hydrochloric acid reacts with magnesium metal, hydrogen gas and aqueous magnesium chloride are produced. What volume of 9.0 M HCl is required to react completely with 5.00 g of magnesium?
Iron reacts with hydrochloric acid to produce iron (2) chloride and hydrogen gas.Fe (s)+ 2 HCL (aq) -FeCl2 (aq) + H2 (g).The hydrogen gas from the reaction 2.2g of iron with excess acid is collected in a 10L flask at 25 degrees celcius. What is the
Iodine is sparingly soluble in pure water. However, it does `dissolve' in solutions containing excess iodide ion because of the following reaction: I-(aq) + I2(aq)= I3-(aq) K = 710. For each of the following cases calculate the equilibrium ratio of [I3-]
a mixture of 10cm3 of methane and 10cm3 of enthane was sparked with an excess of oxygen. after coolin to room temp, the residual gas was passed through aq KOH. what volume of gas was absorbed by the alkali ? Write the equations for CH4 + O2 and C2H6 + O2.
The reaction for the burning of one type of match tip is as follows: P4S3(s) + 8 O2(g)----> P4O10(g) + 3 SO2(g) What volume in L of SO2 at STP can be produced by the burning of 1.00 g P4S3 in excess O2?
Calculate volume of Carbon dioxide produced on heating 10g of limestone at S.T.P
Calculate the volume of Sulfur dioxide produced when 27.9 mL of O2 reacts with carbon disulfide
1.How many grams of carbon monoxide are needed to react with an excess of iron (III) oxide to produce 198.5 grams of iron? Fe2O3(s) + 3CO(g) ----- 3CO2(g) + 2Fe(s) Show all work! 2.Hydrogen gas can be made by reacting methane (CH4) with high temperature
The chemical substance in natural gas is a compound called methane. Its molecules are composed of carbon and hydrogen and each molecule contains four atoms of hydrogen and one atom of carbon. In this compound, 0.33597g of hydrogen is combined with 1g of
Nitrogen & hydrogen goes react to form ammonia gas as follows: N2(g)+3H2(g)-->2NH3(g) At a certain temperature & pressure, 1.2L of N2 reacts with 3.6L of H2. If all the N2 and H2 are consumed, what volume of NH3, at the same temperature & pressure will be
What is the heat in Joules required to raise the temperature of 25 grams of water from 0 °C to 100 °C? What is the heat in calories? Knowing that 4.18 J = 1 calorie and C= 4.18 J/g·°C M=25g C=4.18 J/g Tf=100 Ti=0 Q=25g x4.18j/g (100-0) Q=25x4.18x(100)
How many tons of zinc can be obtained from 976 tons of zinc ore that is 78.0% zinc carbonate?
What physical property of water and HCl allows us to separate them from the zinc chlorine compound produced in the reaction?
Ammonia is produced by the reaction of hydrogen and nitrogen. N2(g)+3H2(g)→2NH3(g)ammonia How many moles of N2 reacted if 0.65mole NH3 is produced? How many moles of NH3 are produced when 1.2moles H2 reacts?
calculate the volume of the hydrogen that will combine with 40 litres of oxygen to form steam at 150 C and atmospheric pressure
If 0.0900 g of a metal, M, reacts with excess hydrochloric acid to form 5.00*10(exp.)-3 moles of hydrogen gas and a solution of MCl(subscript)3. Calculate the molar mass of metal, M and identify it. The unbalanced equation is: M(s)+ HCl(aq) =>MCl(sub.)3 +
How many grams of zinc metal are required to produce 2.00 L of hydrogen gas at STP according to the chemical equation shown below? Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
a solution is made by dissolving 25 g NaCl in enough water to make 1.0 L solution. Assume that density of the solution is 1.0 g/mL. calculate the mass percent, molarity, molality, and mole fraction of NaCl. help please 25g/58.44g NaCl=.428 mol 1000 grams
Calculate the volume of CO2 produced at S.t.p when 25cm3 of 0.25mol/dm3 Hcl reacts with Na2Co3.
If i have 0.5 mole of hydrogen peroxide how many moles of oxygen would be produced assuming all of the hydrogen peroxide decomposes?
If 96g SO2 is added to 2 moles of oxygen at STP,calculate the volume of SO3 that is formed
A 2.50-L volume of hydrogen measured at -100 degrees Celsius is warmed to 100 degrees Celsius. Calculate the volume of the gas at the higher temperature, assuming no change in pressure.
in an attempt to establish the formula of an oxide of nitrogen , a known volume of the pure gas was mixed with hydrogen and passed over a catalyst at a suitable temperature. 100% conversion of the oxide to ammonia and water was shown to have taken place.
Yes...another calculation problem. Rxn: 1ml isopentyl alcohol + 1.5ml glacial acetic acid + 3 drops sulfuric acid=> isopentyl acetate to calculate the theoretical yield.. I know that the acetic acid is in excess but how would I calculate the theoretical
1. A small piece of zinc reacts with dilute HCl to form H2, which is collected over water at 16°C into a large flask. The total pressure is adjusted to barometric pressure (752 torr), and the volume is 1538 mL. Use Table 5.2 to help calculate the partial
on heating 25g of a saturated solution to dryness at 60c,4g of anhydrous salt was recovered.calculate it's solubility in grammes per 100g of solvent
Hydrogen fluoride is used in the manufacture of Freons (which destroy ozone in the stratosphere) and in the production of aluminum metal. It is prepared by the reaction below. CaF2 + H2SO4 CaSO4 + 2 HF In one process 9.00 kg of CaF2 are treated with an
calculate the volume of gas at STP that is produced when 1g of silver nitrate is heated. the unbalanced reaction is: AgNO3(s)=Ag(s)+NO2(g)+O2(g)
Determine how many mL of solution A (acetic acid-indicator solution) must be added to solution B (sodium acetate-indicator solution) to obtain a buffer solution that is equimolar in acetate and acetic acid. Solution A: 10.0 mL 3.0e-4M bromescol green
Please help! How are acids and protons related? A. The substance with a higher pH has twice as many hydrogen ions per volume of water. B. The substance with the lower pH has 1000 times as many hydrogen ions per volume of water. C. The substance with the
Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s) + 3Cl2(g) -> 2AlCl3(s) You are given 19.0g of aluminum and 24.0g of chlorine gas. a)If you had excess chlorine, how many moles of of aluminum chloride could be
I have a question that I don't understand from my first year chem lab. Calculate the minimum volume of water needed to decompose all the excess Ethanoic Anhydride. Recall: 1.0g of H2O = 1.0 ml of water. How do I go about doing this?
Calculate the volume, in milliliters, of a 0.220 M KOH solution that should be added to 5.750 g of HEPES (MW = 238.306 g/mol, p𝐾a = 7.56) to give a pH of 7.98.
11. Infinitely many different sectors can be cut from a circular piece of paper with a 12-cm radius, and any such sector can be fashioned into a paper cone with a 12-cm slant height. (a) Show that the volume of the cone produced by the 180-degree sector is
1.00 g zinc and 0.80 g sulfur are allowed to react all the zinc is used up 1.50 g of zinc sulfide is formed and some unreacted sulfur remains what is the mass of unreacted sulfur
Given the equilibrium: HCN(aq) + H2O(l) ←→ H3O+(aq) + CN-(aq) ΔH >0; Ka = 4.0 x10-10 What happens to the concentration of hydrogen cyanide [HCN] when the following stresses are placed on the system at equilibrium? NaCl is added ---> Stays the Same but
The value of delata h for the reaction below is -186 kJ. Calculate the heat Kj released from the reaction of 25g of Cl2
Hydrogen gas produced by this reaction is typically collected via water displacement, during which time the hydrogen gas becomes saturated with water vapor. If 238.4 mL of gas with a total pressure 1.27 atm was collected via water displacement at 29.4 °C,
Buffer capacity is a measure of a buffer solution\'s resistance to changes in pH as strong acid or base is added. Suppose that you have 165 mL of a buffer that is 0.360 M in both benzoic acid (C6H5COOH) and its conjugate base (C6H5COO–). Calculate the
How many moles of NH3 can be produced from 19.5mol of H2 and excess N2
What would the molarity of 50 mL of 3% hydrogen peroxide be if it's volume/volume? I know how to do weight/volume but not this, someone help?
The specific heat capacity of zinc is 0.386 J/g ºC . How many joules would be released when 268 grams of zinc at 96.0 ºC were cooled to 28.0 ºC?
8g of hydrogen is burnt in the presence of excess oxygen.the mass of water formed is?
The following reaction represents the decomposition of hydrogen peroxide 2H2O2 -> o2 (g) + 2H2O (l) How many molecules of water are produced from the decomposition of 3.4g of Hydrogen peroxide, H2O2? Please walk me through this one, I need more then just
what mass of H2(g) is produced from the reaction of 5.2g Fe(s) with excess hydrochloric acid?
How many grams of N2 are produced when 15.0 moles of NH3 react with excess NO
A cylinder with a movable piston contains 2.00 of helium,He, at room temperature. More helium was added to the cylinder and the volume was adjusted so that the gas pressure remained the same. How many grams of helium were added to the cylinder if the
When potassium cyanide (KCN) reacts with acids, a deadly poisonous gas, hydrogen cyaninde (HCN) is given off. Here is the equation: KCN(aq) + HCl(aq) ----> KCl(aq)+ HCN(g) If a sample of 0.140 g of KCN is treated with an excess of HCl, calculate the amount
What is the volume in liters of one mole of hydrogen at STP . If 2.73 moles of hydrogen at STP occupies a volume of 61.2 liters
pure zinc metal into a solution of copper(II) sulfate, the zinc will slowly dissolve to produce zinc sulfate solution, and the copper(II) ion of the copper(II) sulfate will be converted to metallic copper. Write the unbalanced equation for this process.
Propane and oxygen react according to the following equation. C3H8(g) + 5O2>>>3CO2(g) + 4H2O(g) Calculate the volume of carbon dioxide and water vapour produced and the volume of oxygen remaining, when 20.0 dm3 of propane reacts with 120.0 dm3 of oxygen.
10g of hydrogen is burnt in the presence of excess oxygen.the mass of water formed is?
Starting out with 50 mL of 0.20 M NaHCO3, calculate how many mL of 0.50 M NaOH solution to add to make 100 mL of approximately 0.10 M (total) buffer solution with a pH of 10.35. By adding NaOH, some of the NaHCO3 gets converted to the conjugate Na2CO3.
how many milliliters of a 0.46 M HCl solution are needed to react completely with a 6.4 g of zinc to form zinc (ii) chloride answer in mL Help please :( I was absent and don't know where to start
In a lab, we added NH3(aq) to CuSO4(aq), and the solution turned dark blue with a precipitate. The problem is that the products ( Cu(NH3)4 and SO4) should be soluble, no? The question is then, what is the percipitate? The ppt is Cu(OH)2. The dark blue
Calculate the volume of .100M NaOH that must be added to reach ph of 3 in the titration of 25.00 mL of .100M HCl
In a constant-pressure calorimeter, 70.0 mL of 0.330 M Ba(OH)2 was added to 70.0 mL of 0.660 M HCl. The reaction caused the temperature of the solution to rise from 21.27 °C to 25.77 °C. If the solution has the same density and specific heat as water,
In a constant-pressure calorimeter, 55.0 mL of 0.310 M Ba(OH)2 was added to 55.0 mL of 0.620 M HCl. The reaction caused the temperature of the solution to rise from 22.23 °C to 26.45 °C. If the solution has the same density and specific heat as water,
In a constant-pressure calorimeter, 60.0 mL of 0.310 M Ba(OH)2 was added to 60.0 mL of 0.620 M HCl. The reaction caused the temperature of the solution to rise from 23.44 °C to 27.66 °C. If the solution has the same density and specific heat as water,
if 100g of iron reacts with excess oxygen, how much rust should be produced?
Calculate the mass of water produced when 3.94 g of butane reacts with excess oxygen. Butane, C4H10, reacts with oxygen, O2, to form water, H2O, and carbon dioxide, CO2, as shown in the following chemical equation: 2C4H10(g)+13O2(g)→10H2O(g)+8CO2(g)
How do I calculate the densities of a hydrogen nucleus and a hydrogen atom?
In a constant-pressure calorimeter, 65.0 mL of 0.320 M Ba(OH)2 was added to 65.0 mL of 0.640 M HCl. The reaction caused the temperature of the solution to rise from 21.98 °C to 26.34 °C. If the solution has the same density and specific heat as water
In a constant-pressure calorimeter, 70.0 mL of 0.340 M Ba(OH)2 was added to 70.0 mL of 0.680 M HCl. The reaction caused the temperature of the solution to rise from 22.00 °C to 26.63 °C. If the solution has the same density and specific heat as water
In a constant‑pressure calorimeter, 70.0 mL of 0.350 M Ba(OH)2 was added to 70.0 mL of 0.700 M HCl. The reaction caused the temperature of the solution to rise from 23.31 ∘C to 28.08 ∘C. If the solution has the same density and specific heat as water
In a constant-pressure calorimeter, 75.0 mL of 0.950 M H2SO4 was added to 75.0 mL of 0.460 M NaOH. The reaction caused the temperature of the solution to rise from 21.13 °C to 24.26 °C. If the solution has the same density and specific heat as water,
How many grams of hydrochloric acid are required to react completely with 4.30 grams of zinc? I got 4.80g HCl for the answer but do not know how to do part 2 which is, How many molecules of a gas will be produced? Thanks.
If 5.00 g of PCl5 is reacted with excess water, how many grams of H3PO4 and HCl would be produced?
How many liters of chlorine gas can be produced when 0.98 L of HCl react with excess O2 at STP?
Fe(S)+ 2 HCl(ag) --> FeCL2(ag)+ H2(g What mass of H2 (g) is produced from the reaction of 5.2 Fe(s) with excess hydrochloric acid?
4. Calculate the mass of zinc carbonate that would remain if 17.0g of zinc carbonate was reacted with 50cm3 of 4M nitric acid. The equation of the reaction is: ZnCO3 (g) + 2HNO3 (aq) Zn (NO3) 2 + CO2 (g) + H2O (l) (Zn=65.4, C=12.0, O=16.0) A certain
So the question I have is: Calculate the pressure of dry hydrogen collected. (Use the water temperature). And the evidence that we obtained was: Length of magnesium 3.8Cm Mass of 1 m of magnesium 1.254g Volume of hydrogen collected 67mL Air temperature 27C
A 0.250-g sample of a magnesium-aluminum alloy dissolves completely in an excess of HCl (aq) . When the liberated H2 (g) is collected over water at 29 degrees celsius and 752 torr, the volume is found to be 301 mL . The vapor pressure of water at 29
A piece of metal has a volume of 20 cm^3 and a mass of 300g.Calculate the density of the metal in kg/m^3.i got 15.plz confirm my answer.And how does one go about this.2.5 litres of water density 1g/cm^3 is added to 8 litres of alcohol density 0.8
Calculate the volume of CO2 that would be produced from 0.5 mole of Fe2O3 according to the equation.Fe2O3(s)+3CO(g)=2Fe(s)+3CO2(g). (1mole of a gas occupies 22.4dm3 at s.t.p)
Calculate the amount of energy in the form of heat that is produced when a volume of 3.56 L of SO2(g) is converted to 3.56 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal gas behavior.
How many grams of hydrogen are released by the reaction of 1.00 g of aluminum with excess potassium hydroxide solution assuming 100% yield

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Some commercial drain cleaners contain sodium hydroxide (NaOH) and powdered aluminium (Al). When the mixture is poured into a clogged drain the reaction given by the following balanced equation occurs: 2Al + 2NaOH + 6H2O → 2NaAl(OH)4 + 3H2 The heat
the chlorine in a 0.12g sample of 95% pure magnesium chloride is to be precipitated as silver chloride, calculate the volume of 0.100m of silver nitrate solution required to precipitate the chloride and give a 100% excess.
Calculate the volume of nitrogen gas that will be produced in the air bag of a car when 88,8g of sodium azide is thermally decomposed at 22 C to give the bag a pressure of 1,10 atm
Given these chemical reactions: Ca^(2+)(aq) + 2IO3^(-)(aq) → Ca(IO3)2(s) Ca(NO3)2·4H2O(s) → Ca^(2+)(aq) + 2NO3^(-)(aq) + 4H2O(l) KIO3(s) → K^(+)(aq) + IO3(-)(aq) Calculate the masses of Ca(NO3)2·4H2O(s) and KIO3(s) required to make 10 g of
The solubility of zinc oxalate is 7.9 x 10 ^-3 M at 18 degrees C. Calculate its Ksp.
Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO (g) + 2H2 (g) -> CH3OH (g) An equilibrium mixture in a 2.50 L vessel is found to contain 2.62e-2 mol CH3OH, 0.170 mol CO, and 0.303 mol H2 at 500 K.
How many grams of PI3 could actually be produced from 250 g of I2 and excess phosphorous if the reaction gives a 98.5% yield? P4 + 6I2 --> 4PI3
4NH3+7O2 yields 4NO2+6H2O If 8g of NH3 reacted with excess O2, how many g of H2O will be produced?
A mixture of 25.0g of NO and an excess of O2 reacts according to the balanced equation. 2 NO + O2→2NO2. How many liters of NO2 are produced at STP?
The volume of an irregularly shaped solid can be determined from the volume of water it displaces. A graduated cylinder contains 19.9mL of water. When a small piece of galena is added, it sinks and the volume increases to 24.5mL. What is the volume of the
If 6.5g of zinc reacts with 5.0g of HCL,according to the reaction.Zn + 2HCL:zncl2+h2 Which substance is the limiting reaction? How many grams of the reactant remains unreactant? How many grams of hydrogen would be produce?
when ammonia is added to Zn(NO3)2 solution, a white precipitate forms, which dissolves on the addition of excess ammonia. But when ammonia is added to a mixture of Zn(NO3)2 and NH4NO3, no precipitate forms at any time. Suggest an explanation for this
What is the maximum mass(g) of KCL that can be added to 1.00L of a 0.0100 M lead(ii) chloride solution without causing any precipitation of PbCl2? Assume the additional KCl does not affect the volume of the solution. For, PbCl2, Ksp=1.6x10^-5 Personally
2CH3OH(l)+3O2(g)→2CO2(g)+4H2O(g Part B Calculate the standard enthalpy change for the combustion of 1 mol of liquid methanol, assuming H2O(g) as a product. Part C Calculate the heat produced by combustion per liter of methanol. Methanol has a density of
in the laboratory, concentrated hydrogen chloride acid reacted with aluminium. hydrogen gas evolved was collected over water at 25 degree celcius and had a volume of 355 centimetre cube at a total pressure of 750mmHg.(the vapour pressure of water at 25
10g of nacl were added to 10ml of water. he resulting solution was diluted to be a final volume of 250ml. Calculate the molarity of the solution. My calculation 10g/58g/mol = 0.173M 0.173M/025L =0.689M Given the density of the solution is 0.9864g/ml.
6.0g of cobolt (II) carbonate was added to 40cm3 of hydrochloric acid, concentration 2.0 mol/dm3. Calculate the maximum yield of cobalt (II) choloride-6-water and show that cobalt (II) carbonate was in excess. CoCO3 +2HCl = CoCl2 +CO2 + H2O CoCl2 + 6H2O =
If 10g of NO react with 20g of O2, what is the maximum amount of NO2 that can be produced? How do I know exactly which is limiting and which is excess, is there a calculation that shows this?
Consider the reaction 2D2(g)+O2(g)→2D2O(l) What is the mass of heavy water, D2O(l), produced when 3.75g of O2(g) reacts with excess D2(g)?
For my lab, I have been asked to calculate the pKa of an unknown amino acid. We titrated the unknown amino acid with NaOH. The pKa needs to be calculated using the Henderson Hasselbach Equation. Obviously you can just get the pH from any point on the graph
hydrogen gas can be produced by reacting aluminum with sulfuric acid .How many L hydrogen gas are produced by reacting 15.0 mol of sulfuric acid with 15.0 mol of aluminum at STP?
Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s) + 3Cl2(g) -> 2AlCl3(s) You are given 19.0g of aluminum and 24.0g of chlorine gas. a)If you had excess chlorine, how many moles of of aluminum chloride could be
In a constant-pressure calorimeter, 60.0 mL of 0.330 M Ba(OH)2 was added to 60.0 mL of 0.660 M HCl. The reaction caused the temperature of the solution to rise from 21.71 °C to 26.21 °C. If the solution has the same density and specific heat as water,
The specific heat of zinc is 0.096 cal/(g °C). Determine the energy required to raise the temperature of 26.1 g of zinc from room temperature (20.0 °C) to 150 °C.
Write the anodic reaction for the electrolysis of concentrated zinc chloride solution. (a) Using plantium electrodes. (b) Using zinc electrodes
A sample of hydrogen gas was collected over water at 36°C and 855 mmHg. The volume of the container was 6.50 L. Calculate the number of moles of H2 collected. (Vapor pressure of water is 44.6 torr at 36°C)
74. Sodium hydrogen carbonate is also known as baking soda. When this compound is heated, it decomposes to sodium carbonate, carbon dioxide, and water vapor. Write the balanced equation for this reaction. What volume of carbon dioxide gas at 77 degrees C
When chlorine gas is added to an aqueous solution of sodium fluoride (aq) a) fluorine gas is produced. b) a synthesis reaction takes place. c) no reaction occurs. d) sodium chloride is produced.
Suppose if 50.0 mL of 0.250 M CoCl2 solution is added to 25ml of 0.35M NicL2 solution. Calculate the concentration in moles per litre, of each of the ions present after mixing. Assuming that the volume are additive.
The reaction of the molecules to produce ethane is C2H4(g) + H2(g) ÃƒÂ¢Ã¢â‚¬Â Ã¢â‚¬â„¢ C2H6(g). A mechanism for this reaction is shown below: (The figures show how the ethene molecule with two hydrogen molecules attached 'binds' to
A solution contains 1.694 mg of CoSO4 (MW 155.0) per mL. Calculate a) The volume of 0.008640 M EDTA needed to titrate a 25.00 ml aliquot of this solution. Step 1. 0.001694g * 25ml * 1/155 g/mol= 0.0002732 mol Step 2. Volume of EDTA needed = 0.0002732 mol/
A 2.52g sample of a compound containing only carbon, hydrogen, nitrogen, oxygen, and sulfur was burned in excess O to yield 4.36g of CO2 and 0.892g of H20. Another sample of the same compound of mass 4.14g, yielded g of SO3. A third sample, of mass, 5.66g,
Hi there - I'm going to post the question as written in my book. Three 20.0 mL samples of nitric acid are titrated with a 0.200 mol/L solution of sodium hydroxide. The results for the three trials are shown in the table below. What is the concentration of
The following reaction represents the decomposition of hydrogen peroxide: 2H2O2 -> O2 (g) + 2H2O (l) How many molecules of water are produced from the decomposition of 3.4g of hydrogen peroxide, H2O2? Please help, I got 0.02 molecules of water but need to
1.06g of sodium trioxocarbonate(iv) reacted with excess dilute 0.1M hydrochloric acid, after the reaction, the unreacted acid required 24cm3 of 0.1M sodium hydroxide for its complete neutralization. Calculate the original volume of the hydrochloric acid
A cylinder with a movable piston contains 2.00g of helium, He, at room temperature. More helium was added to the cylinder and the volume was adjusted so that the gas pressure remained the same. How many grams of helium were added to the cylinder if the
An alloy is made by using copper and zinc in the ratio of 17:3 how much zinc is used to make 4kg of the alloy?
A 25g piece of an unknown metal alloy at 150 degrees Celsius is dropped into an insulated container with 200 g of ice. Calculate the specific heat capacity of the metal, given that 9.0 g of ice melted. How would you work this out?
2H2O --> 2H2 + O2 if 30 mL of hydrogen in the above reaction, how many milliliters of oxygen are produced?
2. Let R be the region of the first quadrant bounded by the x-axis and the cuve y=2X-X^2 a. Find the volume produced when R is revolved around the x-axis b. Find the volume produced when R is revolved around the y-axis
Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen, and methane. 2 NH3(g) + 3 O2(g) + 2 CH4(g) 2 HCN(g) + 6 H2O(g) If 5.00 x 10^3 kg each of NH3, O2, and CH4 are reacted, what mass of HCN and of H2O will be produced,
Calculate the number of grams of sulfuric acid in 1 gallon of battery acid if the solution has a density of 1.25g/mL and is 38.3{\rm \\%} sulfuric acid by mass.
An equilibrium mixture contains 0.250 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container. CO(g) + H2O(g) CO2(g)+ H2(g) How many moles of carbon
Given a 1.00 L solution that is 0.60 M HF and 1.00 M KF, calculate the pH after 0.080 mol NaOH is added, and calculate the pH after 0.24 mol HCl is added to the original solution.
A solution of the weak acid HA was titrated with 0.100 M NaOH. the pH measured when vb=ve was 4.62 mL was 4.62 mL. Calculate the Ka of weak acid. (vb= added base volume, ve= equivalence point reading)
N2 + 3H2 --> 2NH3 If 28 grams of nitrogen reacts with excess hydrogen, how many grams of NH3 will be formed?
1.Hydrogen gas can be made by reacting methane (CH4) with high temperature steam: CH4(g) + H2O(g) ----- CO(g) + 3H2(g) How many hydrogen molecules are produced when 256 grams of methane reacts with steam? 2. Ammonia (NH3) reacts with oxygen (O2) to produce
Zinc carbonate dissolves in water to the extent of 1.12 x 10-4 g/L at 25 C. Calculate the solubility product Ksp for ZnCO3 at 25 C.
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: 2 C 6 H 5 Cl (Chlorobenzene) + C 2 H O Cl 3(chloral) ==> C 14 H 9 Cl 5 (DDT) + H 2 O In a government lab, 1142 g of chlorobenzene is reacted with 485g of
If water I'd added to magnesium nitride, ammonia gas is produced when the mixture is heated Mg3N2 (s) + 3H2O (l) ----> 3MgO) (s) + 2NH) (g) *Only the numbers at the beginning aren't subscripts* If 10.3 g of magnesium nitride is treated with water, what
when a quantity of powdered sulphur is burnt in excess oxygen, 100cm3 of SO2 were produced at STP CAL,the vol of gas at STD
Calculate the change in PH when 6 ml of 0.1 M HCl is added to 100 ml of a buffer solution that is 0.1 M in NH3 and 0.1 M in NH4Cl. And calculate the change in PH when 6 ml of 0.1 M NaOH is added to the original buffer solution.
1. How many molecules of ammonia, NH3, are produced from 12.5 grams of hydrogen in the following balanced equation?
Suppose a substance has been prepared that is composed of carbon, hydrogen, and nitrogen. When 0.1156 gram of this compound is reacted with oxygen, 0.1638 gram of carbon dioxide (CO2) and 0.1676 gram of water (H2O) are collected. Assuming that all the
Calculate the mass of hydrochloric acid needed to react with 5.00 moles of zinc in a single replacement reaction.
Consider the reaction: 2CH4(g) + 3O2(g) + 2NH3(g) --> 2HCN(g) + 6H2O(g) If 203.5 g NH3 is reacted with excess CH4 and O2, what mass in grams of HCN can be produced?
How many grams of ammonia are formed when 1.34 grams of nitrogen react with an excess of hydrogen(3 H2 + N2 reacts to form 2 NH3)(Answer to tenths ex. 2.5)?
1. As the pressure of an enclosed gas decreases to half its original value, what happens to the volume of the gas if temperature is held constant?(1 point) The volume decreases to half of its original value. The volume decreases to one-fourth of its
Hydrogen sulfide, H2S, is a foul-smelling gas. It burns to form sulfur dioxide. 2H2S9(g) + 3O2(g) → 2SO2(g) + 2H2O(g); ∆H = -1037kJ Calculate the enthalpy change to burn 36.9g of hydrogen sulfide
Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag+ ion in the solution after equilibrium has been reestablished. For AgCl, Ksp = 1.8 × 10¯10
How many grams of ammonia are produced when 6.50 mol hydrogen reacts with nitrogen? 3H2 + N2 2NH3
2. Methane (CH4), ammonia (NH3), and oxygen (O2) can react to form hydrogen cyanide (HCN) and water according to this equation: CH4 + NH3 + O2  HCN + H2O You have 8 g of methane and 10 g of ammonia in excess oxygen. Answer the following questions: •
12. What balances charges that may build up as reduction and oxidation occur in a voltaic cell? *the salt bridge one of the half-cells the electrolyte solutions the moving electrons 13. What is the electrode in the center of the most common dry cell made
2. Methane (CH4), ammonia (NH3), and oxygen (O2) can react to form hydrogen cyanide (HCN) and water according to this equation: CH4 + NH3 + O2  HCN + H2O You have 8 g of methane and 10 g of ammonia in excess oxygen. Answer the following questions: •
3. Methane (CH4), ammonia (NH3), and oxygen (O2) can react to form hydrogen cyanide (HCN) and water according to this equation: CH4 + NH3 + O2  HCN + H2O You have 8 g of methane and 10 g of ammonia in excess oxygen. Answer the following questions: •
Can you please tell me if these are correct? 1. Sodium Hydrogen Sulfite reacts with hydrochloric acid to produce sulfur dioxide gas, water and sodium chloride NaHSO3 + HCl -----> SO2 + H2O + NaCl 2. Sodium nitrate reacts with hydrochloric acid to produce
A 25 ml sample of household bleach was diluted to 500 ml in a volumetric flask. An unmeasured excess of potassium iodide was aded to a 20 ml aliquot of the diluted sample; the iodine liberated in the reaction: OCl- + 2I- -> I2 + Cl- + H2O required 34.5 ml
I need some help finding the net ionic equation for these two problems: 1. Bromine is added to a dilute solution of sodium hydroxide. 2. Sulfuric acid is added to a solution of lithium hydrogen carbonate. This is what I have for reactants: Br2 + NaOH and
How many grams of NH3 can be produced from 2.89mol of N2 and excess H2. Express your answer numerically in grams.
In a constant-pressure calorimeter, 50.0 mL of 0.300 M Ba(OH)2 was added to 50.0 mL of 0.600 M HCl. The reaction caused the temperature of the solution to rise from 24.50 degrees C to 28.59 degrees C. If the solution has the same density and specific heat
what volume of gas at 40°C and 1.50 atm is necessary to react with 300 L of hydrogen gas measured at the same conditions? 2H2 (g) + O2 (g) --> 2H20 (g) 1.50 atm= 151.KPa How would I solve this? Because I can't use: PV = nRT I have pressure, temperature,
We did the gold penny lab, where we bathed a copper penny in a hot zinc-NaOH mixture to turn it a silver color, then we heated that in a flame to turn it a gold color. There are two questions that go with this lab that I don't understand, however: 4. Did
Hey bob- Here's what I got so far: 3AgNO3 + Na3PO4 ---> Ag3PO4 + 3NaNO3 Silver nitrate and sodium phosphate are reacted in equal amounts of 200. g each. How many grams of silver phosphate are produced? 1. What is the limiting? 2. How much silver phosphate
Strong base is dissolved in 665 mL of 0.400 M weak acid (Ka = 3.69 × 10-5) to make a buffer with a pH of 3.94. Assume that the volume remains constant when the base is added. HA(aq) + OH-(aq) -> H2O(l) + A-(aq) Calculate the pKa value of the acid and
calculate the number of moles of Al2O3 that are produced when .60 mol of Fe is produced in the following reaction. 2Al(s) +3FeO = 3Fe(s) + Al2O3(s)
A rock salt (NaCl), ice, and water mixutre is used to make homemade ice cream. How many grams of rock salt must be added to lower the freezing point 10.0 degrees C? I have no idea what to do, please help! delta T = Kf*i*m delta T = 10. Kf is the molal
If 6.64 moles of C5H12 reacts with excess O2, how many moles of CO2 will be produced in the following combustion reaction? Can plz explain how to do it Thank You
When 1.2 x 10^-3 mol of nitric acid react with excess sodium carbonate, how many moles of carbonic acid are produced?
how many grams of CO2 are produced when 88 grams of O2 are reacted with an excess of butane?
Consider the following equilibrium reaction: NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g) When 100 g of sodium hydrogen carbonate are added to a reaction vessel, the temperature is increased to 200°C, and the system comes to equilibrium. What happens to the
How many litres of hydrogen at 0 celsius and 1400 mm Hg are produced if 15g of magnesium reacts with sulphuric acid
2Al+3H2SO4⟶3H2+Al2(SO4)3 what mass of hydrogen is produced from 4.55 mol of aluminum?
What mass of NH4Cl must be added to 0.750 L of a 0.1M solution of NH3, to give a buffer solution with a pH of 9.26? (Hint: Assume a negligible change in volume as the solid is added.) Kb of NH3 = 1.8 x10-5 %3D Kw= 1 x 10-14
What mass of NH4Cl must be added to 0.750 L of a 0.100 M solution of NH3 to give a buffer solution with a pH of 9.26? Kb(NH3) = 1.8 x 10^-5. (Hint: Assume a negligible change in volume as the solid is added.)
Sodium carbonate reacts with hydrochloric acid as shown below in an unbalanced chemical equation. What mass of CO2 is produced from the reaction of 2.94g Na2CO3 with excess HCL?
Which of the following statements is (or are) true? I Hydrogen bonds occur between two hydrogen atoms. II Hydrogen bonding occurs between a hydrogen atom and an oxygen atom within a molecule. III Hydrogen bonding requires a molecule containing a large
An unknown compound contains only carbon, hydrogen, and oxygen . Combustion of 2.50 g of this compound produced 3.67 g of carbon dioxide and 1.50 g of water. What is the empirical formula of a substance that contains 8.33×10−2 mol of carbon, 0.167 mol
Which element would have a full outer shell of electrons if it gained three electrons? boron lithium nitrogen argon THIS ONE Which statement best explains why hydrogen's atomic number is equal to its mass? hydrogen is in the first row and the first column
Consider the chemical reaction C + H2O -----> CO + H2 How many liters of hydrogen gas are formed From the complete reaction of 1.07 mol of C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and the temperature of 315K So I'm looking for
Three volatile compounds X,Y, and Z each contain elements Q. The precent by weight of element Q in each compound was determined. Some of the data obtained are given below Percent by weight Molecular Compound of Element Q Weight X 64.8% ? Y 73.0% 104. Z
The overall reaction in a commercial heat pack can be represented as shown below. 4 Fe(s) + 3 O2(g) 2 Fe2O3(s) ΔH = -1652 kJ How much heat is released when 4.00 mol iron is reacted with excess O2? How much heat is released when 1.00 mol Fe2O3 is produced?
An unknown compound contains only carbon, hydrogen, and oxygen (CxHxOx). Combustion of 3.50G of this compound produced 5.13G of carbon dioxide and 2.10G of water A.How many moles of carbon, , were in the original sample? b. How many moles of hydrogen, ,
I am confused on how to do the last question. Calculate molarity of HCl from the volumes of acid and base at the equivalence point and the molarity of NaOH from the titration curve. (M of Acid)x(v of acid)= (m of base)x(v of added base) M1= 0.50M of NaOH x
How many grams of aluminum chloride are produced when 18 g of aluminum are reacted with an excess of hydrochloric acid? 2AL(s) + 6HCl(aq) ---> 2AlCl3(aq) + 3H2(g)
A mass of ideal gas of volume 400 cm3 at a temperature of 27 ˚C expands adiabatically until its volume is 500 cm3. Calculate the new temperature. The gas is then compressed isothermally until its pressure returns to the original value. Calculate the final
nitrogen and hydrogen react in the haber process to form ammonia. All substances are in the gas phase. If 0.385atm of nitrogen and 0.792 atm of hydrogen react, what is the partial pressure of ammonia(in mmHg) when this reaction goes 67 complete. The volume
One alloy of brass is 70% copper and 30% zinc. Another alloy of brass is 40% copper and 60% zinc. How many grams of each of these alloys need to be melted and combined to obtain 300 grams of a brass alloy that is 60% copper and 40% zinc
13. Solid sodium reacts violently with water, producing heat, hydrogen gas, and sodium hydroxide. How many molecules of hydrogen gas are formed when 48.7 g of sodium are added to water? 2Na + 2H2O = 2NaOH + H2 So far I have this much figured out: Mass to
What mass in grams of sodium hydroxide is produced if 20.0 g of sodium meal reactts with excess water according to the chemical equation 2 Na(s)+2 H2O(l)=2 NaOH(aq)+H2(g)?
If you reacted 100.0 g of carbon tetrachloride (CCl4) with excess antimony fluoride (SbF3), how many grams of carbon dichloride difluoride would be produced?

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If 50.0 g of silicon dioxide is heated with an excess of carbon, 27.9g of silicon carbide is produced. SiO2(s) + 3C(s) --> SiC(s) + 2CO(g) what is the percent yield of this reaction?
A zinc-copper battery is constructed as follows at 25°C. Zn|Zn^2+ (0.15 M)||Cu2+(3.00 M)|Cu The mass of each electrode is 200. g. a) Calculate the cell potential when this battery is first connected. - i got this to be 1.14V b.) Calculate the cell
one of the properties of matter is density. density is defined as the mass per unit of volume of a substance. a substance that is more dense than another has more mass for the same volume than the other substance. Density of gases : chlorine-3.21,
Nitric acid can be produced from NH3 in three steps process: I)4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) II)2NO(g) + O2(g) → 2NO2(g) III)3NO2(g) + H2O(l) →2HNO3(aq) + NO(g) % yield of Ist, IInd & IIIrd are respectively 50 % , 60 % & 80 % respectively the
a) A 750-mL sample of hydrogen exerts a pressure of 822 torr at 325 K. What pressure does it exert if the temperature is raised to 475 K at constant volume? b) Aluminum oxide, Al2O3, is used as a filler for paints and varnishes as well as in the
Hydrochloric acid(75.0 ml of 0.250 M) is added to 225.0 ml of 0.0550 M Barium hydroxide solution. What is the concentration of the excess H+ or OH- ions left in this solution?
Analysis questions: A) What evidence is there that the gas bubbles formed in the first part of the investigation were hydrogen gas? Answer: Evidence there was that proved that the gas bubbles formed in the first part of the investigation were hydrogen gas
If tums is added to 20.0 mL of 0.400 M HCl solution, how many grams of CO2 gas are produced?
five hundred kcal of heat is added to 2-kg of water at 80 degree Celsius. how much steam is produced?
Liquid water can be separated into hydrogen gas and oxygen gas through electrolysis. 1 mole of hydrogen gas and 0.5 moles of oxygen gas is produced from 1 mole of liquid water collected in separate 10 L containers at 1 atm. Will the temperatures of the
If 10.5 g of hydrogen, H2, were mixed with 6.51 g of acetylene, C2H2, and allowed to react according to the following equation, what is the theoretical yield of ethane,C2H6 produced.
A zinc-copper battery is constructed as follows. Zn | Zn2+ (0.70 M) || Cu2+ (2.30 M) | Cu The mass of each electrode is 200. g. (a) Calculate the cell potential when this battery is first connected. 1 V (b) Calculate the cell potential after 10.0 A of
When 22.50 mL of 0.500 M H2SO4 is added to 22.50 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate ΔH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the
mass of empty flask with stopper = 32.634 g mass of flask with water and stopper = 59.479 g density of the water = 0.9973 g/cm^3 mass of water = 26.845 g volume of water = 26.918 cm^3 the flask is then emptied and an unknown substance is added mass of
Consider a 1.50-g mixture of magnesium nitrate and magnesium chloride.After dissolving this mixture in water,0.500M silver nitrate is added dropwise until precipitate formation is complete. THe mass of the white precipitate formed is 0.641 g. a)Calculate
A buffer solution contains .4mol of formic acid, HCOOH and a .6mol of sodium formate, HCOONa, in 1L of solution. Ka of formic acid is 1.8 x 10^-4. a) calculate pH b) if 100ml of this buffer solution is diluted to a volume of 1L with pure water, the pH does
Given the following balanced equation, determine the mass of iron metal that would be produced from the complete reaction of 94.7g of aluminum with excess iron II oxide. 2 Al(s) + 3FeO(aq) → 3Fe(s) + Al2O(aq)
How many moles of aluminum oxide can be produced from 12.8 moles of oxygen gas (O2) reacting with excess aluminun (Al)? useing this equation: ---- I don't get how to do these? 4Al(s) + 3O2--> 2Al2O3(s)
Strong base is dissolved in 675 ml of 0.200 m weak acid (ka=3.25x10^-5) to make a buffer with a ph of 3.95. Assume that the volume remains constant when the base is added. HA + OH ---> H2O + A^- calculate the pka value of the acid and determine the number
A volume of 2.0 L of He at 46 degrees celsius and 1.2 atm of pressure was added to a vessel that contained 4.5 L of N2 at STP. What is the total pressure and partial pressure of each gas at STP after the He is added?
It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy for an atom of hydrogen, making the assumption that ionization is the transition from n=1 to n=infinity. I don't know how to solve this
calculate the change in pH when 9.00ml of 0.100M HCl(aq) is added to 100.0mL of a buffer solution that is 0.100M in NH3(aq) and 0.100M NH4Cl(aq). ...Calculate the change in pH when 9.00,L if 0.100M NaOH(aq) is added to the original buffer solution.
When heated to 350. ∘C at 0.950 atm, ammonium nitrate decomposes to produce nitrogen, water, and oxygen gases: 2NH4NO3(s)→Δ2N2(g)+4H2O(g)+O2(g) Using the ideal gas law equation, calculate the volume, in liters, of water vapor produced when 21.8 g of
Determine the theoretical and percent yield of hydrogen gas is 36 g of water undergoes electrolysis to produce hydrogen and oxygen and 3.8 g of hydrogen is collected.
calculate the mass in grammes of copper that will be deposited by dissolving 6.5g of zinc in copper tetraoxosulphate(vi) solution
In the chemical reaction, . Zn(s) + CuSO4(aq) �¨ ZnSO4(aq) + Cu(s), (A) metallic zinc is the reducing agent. (B) metallic zinc in reduced. (C) copper ion is oxidized. (D) sulfate ion is the oxidizing agent.
1. An 887.0 mg sample of a mixture containing only NaCl and KCl is dissolved in water, and excess AgNO3 is added to yield 1.913 g of AgCl. Compute the mass-% of each compound in the mixture.
Consider the titration of 80.0 mL Ba(OH)2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added. a.) 0.0 mL *Which molecular equation do I use? b.) 20.0mL Ba(OH)2__+2HCl_+=>+_BaCl2_+____2HOH 80.0
Before 1982 the US Mint cast penny coins from a copper and zinc mixture. If a 1980 penny weighs 3.051g and contains 0.153g zinc, what is the percent of copper in the coins?
When Pb-208 bombarded with Ni-64, a new element and six neutrons are produced. What isotope of the new element is produced by this reaction? Question 17 options: Ds-266 Ds-272 Rf-266 Rf-272 I believe it is either rf- 272 or Ds-272 because i added 208+64,
Fe3O4 reacts with CO according to the equation Fe3O4 + 4CO => 4CO2 + 3Fe If 478.9 g Fe3O4 is reacted with excess CO, what mass of CO2 will be produced?
A worm has a diameter of 2.4cm and its length is upto 1.9M. a)How do I calculate the surface area? b)How do I calculate the volume? c)How do I work out the volume ratio of the worm? Please help! Thanx kim xxx Surface area= PI*2*radius * length] Volume= PI
In an experiment 3.10g of carbon, hydrogen and oxygen produced 4.4g of C02 and 2.7g of water on complete combustion. Determine the empirical formula of the compound ( C= 12, 0= 16, H =1)
C2H6(g) C2H2(g) + 2 H2(g) The ΔH° for the reaction above is +312 kJ. The system is initially at equilibrium. In which direction will the reaction shift in each of the following situations? e) The temperature is decreased. g) He is added at constant
Zinc carbonate, ZnCO3(s), dissolves in water to give a solution that is 1.7 multiplied by 10-5 M at 22°C. Calculate Ksp for ZnCO3(s) at this temperature.
Magnesium metal reacts with phosphoric acid to produce hydrogen gas. If 50 g of phosphoric acid is used, how much magnesium metal is needed? How much hydrogen gas is produced?
I'm posting this again today hoping someone can clarify this for me-I've posted it prior but no one answered yesterday so I'll try again. Thank you in advance I have two question 1.In a dehydration synthesis reaction which of the following occur- a.
what is the percent yield of reaction in which 455g of tungsten (VI) oxide (WO3) reacts with excess hydrogen gas to produce metallic tungsten and 9.60 cm^3 of water.(density of water = 1.00 g/cm^3) ???
Zn + 2HCl ---> ZnCl2 + H2(g) What mass of zinc is needed to produce 115 mL of hydrogen? t's given 115 mL of hydrogen, so can convert to 115/1000/22,4 = 0.0051 moles H2 - the ratio between HCl and H2 is 2 : 1, so the moles of HCl needed for this reaction is
Hydrogen peroxide decomposes to water and oxygen gas by the following reaction 2H2O2(l) → 2H2O(l) + O2(g) If 30 g of hydrogen peroxide decomposes completely, what volume of oxygen gas is formed at STP? 1. 19.77 L 2. 22.41 L 3. 9.89 L 4. 10.79 L 5. 24.46
a 5.000ml aqueous sample containing hydrogen peroxide as diluted to 25ml and analyzed by titration with permanganate. 2MnO4- + 5H2O + 6H+ --> 5O2 + 2Mn^2+ + 8H2O The sample required 42.8 mL of 0.0175 M permangante to reach the end point. What is the
calculate the mass of potassium hydrogen phthalate needed to prepare a 0.1M solution in a 250 ml volumetric flask given that the molar mass of potassium hydrogen phthalate is 204,23g/mol
When 84.8 g of iron(III) oxide reacts with an excess of carbon monoxide, iron is produced. Fe2O3(s) + 3CO(g) ==> 2Fe(s) + 3CO2(g) what is the theoretical yield of iron?
What is the molarity of ZnCl2 that forms when 30.0g of zinc completely reacts with CuCl2 according to the following reaction? Assume a final volume of 285 mL. Zn(s) + CuCl2(aq)--> ZnCl2(aq) + Cu(s) Please Explain!! Thanks!!
Brass is an alloy formed from copper and zinc in the ratio 3:2, based on weight. If 120g of copper is needed for a certain piece of brass, how much zinc will be needed?
Calculate how many moles of Na2S2O3 must be added to dissolve 0.020 mol AgBr in 1.0 L of water at 25°C (assume constant volume). AgBr(s) ↔ Ag+(aq) + Br−(aq) Ksp = 3.3 x 10^−13 Ag+(aq) + 2S2O32−(aq) ↔ [Ag(S2O3)2]3−(aq) Kf = 2.0 x 10^13 (1)
Hydrogen iodide reacts with itself to give hydrogen and iodine. The equilibrium constant is about 2.0 x 10─3 at a particular temperature. If you were to place some hydrogen iodide in a container and seal the container, what would you expect to find at
In a constant-pressure calorimeter, 50.0 mL of 0.300 M Ba(OH)2 was added to 50.0 mL of 0.600 M HCl. The reaction caused the temperature of the solution to rise from 21.73 °C to 25.82 °C. If the solution has the same density and specific heat as water,
The amount of trash G (t) , in tons per year, produced by a town is projected to continue growing according to the formula dG/d t = 80 + 4t . Based on this projection, calculate the total amount of trash that will be produced over the next 5 years, with t
Here is the question: sodium hydride reacts with excess water to produce aqueous sodium hydroxide and hydrogen gas: NaH(s)+H2O-->NaOH(aq)+H2(g) A sample of NaH weighing ________g will produce 982mL of gas at 28.0 C and 765 torr, when the hydrogen is
Calculate the new molarity if each of the following dilutions is made. Assume the volumes are additive. (a) 52.3 mL of water is added to 27.1 mL of 0.124 M KOH solution (b) 110. mL of water is added to 54.2 mL of 0.808 M NaCl solution ((please show work,
1. Silicon dioxide reacts with carbon upon heating to produce silicon carbide (SiC) and carbon monoxide. SiO2(s) + 3C(s) = SiC(s) + 2CO(g) a. What mass of carbon is required to react completely with 15.70 g of SiO2? b. When 152 g of SiO2 reacts with excess
1.Cell respiration glucose is reacted wth oxygen in body to produce carbon dioxide and water how many liters of carbon dioxide would be produced if 90.0 g of glucose completely reacts with oxygen C6H12O6(s)+ 6O2(g) -> 6H2O(g) + 6CO2 (g) How many liters of
Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia (NH3). At 200 oC in a closed container, 1.1 atm of nitrogen gas is mixed with 2.1 atm of hydrogen gas in an otherwise empty container. At equilibrium, the total pressure is 2.2 atm. Calculate
From the ideal gas law, calculate the volume per helium atom in a litre of helium gas kept at room temperature and atmospheric pressure. Additionally, calculate the length of the side of a cube with this volume.
I collected questions from my book which I don't understand plz help me I am stuck plzz.!!!!!!!! Three different solutions containing the same solute at the same temperature are made to be saturated. Beaker 1 has 200.0 mL, beaker 2 has 500.0 mL and beaker
A metal shpere with ane excess of 11 electrons touches an identical metal sphere with an excess of 15 electrons. After the spheres touch, the number of excess electrons on the second sphere is? My book tells me it is 13, but I don't understand why. If
The specific heat of zinc is 0.386 J/g degrees Celsius. How many joules would be released when 454 grams of Zinc at 96.0 degrees Celsius were cooled to 28.0 degrees Celsius.
A 0.464 gram sample of a metal, M, reacts completely with sulfuric acid according to: M(s) +H2SO4(aq)=MSO4(aq)+H2(g) A volume of 211 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level.
The reaction of 8 grams of fluorine with excess chlorine produced 6.4 grams of ClF3. What percent yield of ClF3 was obtained? Answer in units of %
The reaction of 5.7 grams of fluorine with excess chlorine produced 7.6 grams of ClF3. What percent yield of ClF3 was obtained? Answer in units of %.
If 3.0 liters of oxygen gas react with excess carbon monoxide at STP, how many liters of carbon dioxide can be produced under the same conditions? 2 CO (g) + O2 (g) ---> 2 CO2 (g)
In the reaction below, 16 g of H2S with excess O2 produced 8 g of sulfur. ? H2S + ? O2 → ? S + ? H2O . What is the percent yield of sulfur? Answer in units of %
4g of a mixture of CaCO3 and sand is treated with an excess of HCl and 0.88g of CO2 is produced. What is the percentage of CaCO3 in the mixture
When NH3 is prepared from 28 g of N2 and excess H2, the theoretical yield of NH3 is 34 g. When this reaction is carried out in a given experiment, only 30 g is produced. What is the percent yield?
What mass, in grams, of sodium hydroxide (NaOH) is produced if 20 grams of sodium metal(Na) reacts with excess water?
Aluminum is produced by the electrolysis of aluminum oxide (Al2O3, bauxite ore) dissolved in molten cryolyte (Na2AlF6). Calculate the mass of aluminum that can be produced in one day in an electrolytic cell operating continuously at 1.0 x 105 amps. The
Consider the titration of 21.0 mL sample of 0.110 M HC2H3O2 with 0.130 M NaOH. what is the initial pH? what is the volume of added base required to reach equivalance point? what is the pH at 5.00 mL of added base? pH at one half o the equivalence point? pH
Ethanoic acid can be reacted with alcohols to form esters, an equilibrium mixture being formed. CH3CO2H + ROH CH3CO2R + H2O The reaction is usually carried out in the presence of an acid catalyst. In an experiment to determine Kc a student placed together
1) A 0.1375-g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 3024 J/C. The temperature increases by 1.126 degrees C. Calculate the heat given off by the burning Mg, in kJ/g and kJ/mol. 2) Determine the
Ammonium nitrate has been used as high explosive because its unstable & decomposes into several gaseous substances. The rapid expansion of the gaseous substances produces the explosive force. NH4NO3-->N2+O2_H2O Calculate the mass of each product gas if
How many moles of ammonia are produced when 2.5 moles of nitrogen are reacted with hydrogen?
Some very effective rocket fuels are composed of lightweight liquids. The fuel composed of dimethylhydrazine (CH3)2N2H2 mixed with dinitrogen tetroxide was used to power the Lunar Lander in its missions to the moon. The two components react according to
What is the standard cell notation for nickel/nickel (II) nitrate and zinc/zinc nitrate?
An ice cube (25g) is at -8.0c how much is required to melt it completly
what mass of H2SO4 is contained in 25g of 15percent w/w solution?
What is the concentration of a solution containing 25g of NaCl in a 250mL sample?"
A person accidentally swallows a drop of liquid oxygen, O2 (l), which has a density of 1.149 g/mL. Assuming the drop has a volume of 0.050 mL, what volume (mL) of gas will be produced in the person’s stomach at body temperature (37 °C) and a pressure of
How many liters of 20 Volume H2O2 will contain one mole of hydrogen peroxide?
An empty relative bottle weighs 25g.it weighs 65g when filled with liquid and 75g when filled with water .calculate the density of the liquid.Take density of the water to be 1000kg
CH3OH(g) ----> CO(g) + 2H2 (g) (delta H =+90.7k) A) is heat absorbed or released in the course of this reaction? b) calculate the amount of heat transferred when 45.0g of CH3OH(g)is decomposed by this reaction at constant pressure. c) for a given sample of
NaN3 is used in some automobile air bags. The impact of a collision triggers the decomposition of NaN3 as follows: 2NaN3(s) to 2Na(s) + 3N2(g). The nitrogen gas produced quickly inflates the air bag between the driver and the windshield. Calculate the
C(s) + H2O(g) + Heat CO(g) + H2(g) 17. How would you adjust the temperature to increase the amount of product? 18. Does the removal of hydrogen gas as it is produced shift the reaction to the left or the right? My last two questions on my homework that I
A balloon is filled with hydrogen at a temperature of 22.0 C and a pressure of 812 mm Hg. If the balloon's original volume was 1.25 liters, what will its new volume be at a higher altitude, where the pressure is only 625 mm Hg? Assume the temperature stays
0.1802 g sample of a chlorocarbon compound was analyzed by burning in oxygen and collecting the evolved gases in a solution of sodium hydroxide. After neutralizing, the sample was treated with 39.50 mL of a 0.025 M AgNO3. This precipitated the Cl- as AgCl
In this case, the inflection point, and equivalence, occurs after 23.25mL of 0.40 M NaOH has been delivered. Moles of base at the equivalence point can be determined from the volume of base delivered to reach the equivalence point and the concentration of
a) Calculate the change in pH when 4.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). b) Calculate the change in pH when 4.00 mL of 0.100 M NaOH(aq) is added to the original buffer
Zn(s) + 2HCl(l)  ZnCl2(s) + H2(g) at STP What mass of zinc is needed to produce 115 mL of hydrogen? - it's given 115 mL of hydrogen, so can convert to 115/1000/22,4 = 0.0051 moles H2 - the ratio between HCl and H2 is 2 : 1, so the moles of HCl needed
In one experiment, the reaction of 1.00 g mercury and an excess of sulfur yielded 1.16 g of a sulfide of mercury as the sole product. In a second experiment, the same sulfide was produced in the reaction of 1.50 g mercury and 1.08 g sulfur . What mass of
A saturated solution of CaSO4(aq) is made in a beaker until there is excess calcium sulfate resting at the bottom. Then solid potassium sulfate is added. Which of the following is true? (The Ksp for potassium sulfate is larger than the Ksp for calcium
Combustion analysis of an unknown compound containing only carbon and hydrogen produced 2.277 g of CO2 and 1.161 g of H2O. What is the empirical formula of the compound? How do I go about solving this?
In one experiment 10.0g NH3 and 10.0g CO2 were combined and allowed to react. Determine how many grams of CH4N2O could be produced and how much of the reactant in excess will remain at the end of the reaction. Chemical equation: 2NH3 + CO2 = CH4N2O + H2O
If a sample contains 25g of carbon14 and 75g of nitrogen14, how many half lives has it undergone
One advantage of the prismoidal formula is that you can use it to a) calculate precise volumes of all prismoids b)calculate both volume and surface area c)determine volumes of figures that are not prismoids d)estimate the volume of solids that are
Nitroglycerin, C3H5(NO3)3, a solid explosive compound, decomposes to carbon dioxide, water vapor, nitrogen, and oxygen. (a) Calculate the total volume of gases when collected at 1.2 atm and 25 degrees Celsius from 2.6*10^2 g of nitroglycerin. (b) What are
Hydrogen accounts for 71% of the Sun's mass today. If only one tenth of that Hydrogen burns into Helium, how long could the Sun keep shining at its present luminosity? Note that Hydrogen fusion has an efficiency of about 0.7% Time in years:
What is the molarity of ZnCl2 that forms when 30.0g of zinc completely reacts with CuCl2 according to the following reaction? Assume a final volume of 285 mL . (please explain step by step I have no clue!) Zn(s) + CuCl2(aq) --> ZnCl2(aq)+ Cu(s)
what mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO3 is added to 20.0mL of 1.00 MNaBr? i keep getting the answer 3.75 g however when i checked in the back of the book it gives me 2.82 g.. can you please explain the universal steps for me
1. Which of the following metals is oxidized by calcium ions? *potassium zinc iron lead 2. The first electrochemical cell was invented by ____. Michael Faraday *Alessandro Volta James Maxwell Benjamin Franklin 3. Why can't a lead storage battery be
Which item is made from a basic ingredient? Soap/ Tea/ Wine/ Vinegar Complete the sentence. When an acid is added to water, hydrogen ions __________. increase decrease stay the same disappear

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What mass of solid aluminum hydroxide can be produced when 50.0mL of .200 M Al(NO3)3 is added to 200.0 mL of .100 M KOH
If we assume the Sun is made totally out of hydrogen, how many hydrogen atoms are contained with the Sun? If the Sun converts half of these hydrogen atoms into helium over its lifetime of about ten billion years, how many hydrogen atoms are converted per
A 2.500×10−2M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.3mL . The density of
How much heat is required to raise the temperature of 25g of aluminum from 25.0 C to 100 C? Convert this value to joules?
n a particular manufacturing plant, two machines (A and B) produce a particular part. One machine (B) is newer and faster. In one five-minute period, a lot consisting of 32 parts is produced. Twenty-two are produced by machine B and the rest by machine A.
What volume of H2 (g) (at 750. mm Hg and 25 C) is produced from 50.0 mL of 0.214 M H2SO4 and 0.300 g of Al?
Hydrogen cyanide, HCN, can be made by a two-step process. First, ammonia is reacted with O2 to give nitric oxide, NO. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) Then nitric oxide is reacted with methane, CH4. 2 NO(g) + 2 CH4(g) → 2 HCN(g) + 2 H2O(g) +
We did not use the volume of the water added initially to the Erlenmeyer in our calculations. Why?
The mass of an empty container is 91 g. The mass of the container filled with water is 111 g. What is the volume of the container? The density of water is 1 g/cm3 .Answer in units of cm3 20cm3 016 (part 2 of 5) 1.0 points The container was emptied, dried,
1. What is the reaction between copper(II) sulfate and barium hydroxide? 2. What is the reaction between thiocyanate and iron(III) nitrate? 3. What is created when hydrogen peroxide is heated? 4. What is produced when HCl and KMnO4 is mixed?
"How many grams of NH3 can be produced from the reaction of 28 g of N2 and 25 g of H2? N2 + 3H2 ---> 2NH3 ==> 28 g N2 x (1 mol N2/14.0 g N2) x (2 mol NH3/1 mol N2) x ( 17.0 g NH3/ 1 mol NH3) = 68 g NH3 25 g H2 x ( 1mol H2/2.0 g H2) x (2 mol NH3/3 mol H2) x
Calculate mass of iron in tablet by spectroscopy? I have to calculate the mass of iron in a tablet..The manufacturers claim it contains 60 mg elemental iron. background info: The tablet was crushed and dissolved in 25ml of 6M Hcl, filtered and added to a
Hi, I did the acid-base titration lab with HCl and 0.5M NaOH. I need to calculate the moles of NaOH from molarity of NaOH and the average volume used. My English isn't good but is it asking me to find the moles of NaOH using the molarity of NaOH and the
The molar mass of a volatile liquid (one which vaporizes easily) can be determined by a the DUMAS METHOD.' In this process a small amount of the liquid (a few drops) is placed in a clean flask. The mouth of the flask is covered with a piece of foil that
If 3.50g of Na3Po4 and 6.40g of Ba(No3)2 are added together how many grams of Ba3(PO4)2 will be produced? Which is the limiting reactant? Please explains step by step THANK YOU
The bad smell of water containing hydrogen sulfide can be removed by the action of chlorine. The reaction is H2S(aq) + Cl2(aq)-->2HCl(aq) + S(s) If the hydrogen sulfide content of contaminated water is 22 ppm by mass, calculate the amount of Cl2 (in grams)
1. Nitrogen gas and sodium liquid are produced by the decomposition of sodium azide NaN3 (s). what volume of nitrogen gas, measured at 25 C and 0.980 atm, is produced by the decomposition of 62.5 g of sodium azide? 2. A gas sample in a container with a
how do I calculate the area occupied by one single molecule, given # of molecules per meter^2 (9.6e15), the Molarity? (.1 m/dm^3) and surface excess? (1.6e-8)
Referring to the following reaction: Pb(NO3)2 (aq) + Na2SO4 (aq) -->PbSO4 (s) + 2NaNO3 (aq) A solution of 0.114 M Pb(NO3)2 with a volume 10.6 mL is added to 12.4 mL of a solution of 0.105 M Na2SO4. Calculate the number of grams of PbSO4 that will form. I
17g of AgNo3 is trated with 25g of HCl. what is the mass of AgCl formed and what is the limiting reagent
How many calories are required at 0 degrees C to melt an ice cube with a mass of 25g? I got 2000 cal. Could you tell me if this is right?
A 100-mL sample of water is titrated with EDTA solutions in problem 2. The same amount of Mg2+ is added as previously, and the volume of EDTA required is 31.84mL. What volume of EDTA is used in titrating the Ca2+ in hard water? Previous answers are: Moles
When surface water dissolves carbon dioxide, carbonic acid (H2CO3) is formed. When the water moves underground through limestone formations, the limestone dissolves and caves are sometimes produced. CaCO3(s) + H2CO3(aq) Ca(HCO3)2(aq) What mass of limestone
What volume of oxygen measured at s.t.p will be produced on heating 24.5g of potassium trioxochlorate (v)?
The volume of CO2 produced by the combustion of 20g of graphite containing 10% impurity will be?
How many grams of Ag2CO3 will precipitate when excess K2CO3 solution is added to 70.0 mL of 0.692 M AgNO3 solution? 2AgNO3(aq) + K2CO3(aq) --> Ag2CO3(s) + 2KNO3(aq)
A given volume of ozone diffused from a certain apparatus in 96seconds calculate the time taken by an equal volume of carbonoxide to diffuse under the same condition?
which two gases have been added to Earth's atmosphere in large amounts and are believed to have increased global warming by absorbing infrared radiation? 1. neon and argon 2. chlorine and nitrogen 3. hydrogen and helium 4. methane and carbon dioxide
what volume of 0.0100 M NaOH must be added to 1.00 L of 0.0500 M HOCl to acheive a PH of 8.00?
CaCO3(s)+2HCl(aq)>CaCl2(aq)+H2O(l)+CO2(g) how many grams of calcium chloride will be produced when 30 g of calcium carbonate are combined with 13 g of hydrochloric acid? Which reactant is in excess and how many grams of this reactant will remain after the
Find the volume of the solid whose base is the region in the first quadrant bounded by y=x^5, y=1 and the y-axis and whose cross -sections perpendicular to the y-axis are equilateral triangles. I don't know what the bounds for the integral would be when I
Reaction 6 1. Place a piece of mossy zinc in a test tube 2 add hydrochloric acid solution to the test tube until the mossy zinc is completely covered What gas was released in reaction 6 and how could you test the gas to confirm its identity?
It turns out that the Van Dar Waals constant b is equal to four times the total volume actually occupied by the molecules of a mole of gas. Using this figure, calculate the fraction of the volume in a container actually occupied by Ar atoms: a) at STP b)
(a) What is the pH of a 2.0 molar solution of acetic acid. Ka of acetic acid = 1.8 x 10¯5 (b) A buffer solution is prepared by adding 0.10 liter of 2.0 molar acetic acid solution to 0.1 liter of a 1.0 molar sodium hydroxide solution. Compute the hydrogen
25g of NH3 is mixed with 4 moles of O2 in given reaction. 4NH3(g)+5O2(g)-->4NO(g)+6H2O(1) Which is limiting reactant?
5.85g of sodium chloride is dissolved in 250mL of solution. Calculate: a)the molarity of the solution b)the mass percentage of the solute. can we use the given volume(i.e,250mL as total volume of the solution or volume of water in this problem?
2H2S + 3O2 → 2H2O +2SO2 given the balanced equation, if 4 moles of hydrogen sulfide react: How many moles of oxygen consumed? How many moles of water and sulfur dioxide are produced?
At stp what volume of SO2 gas will be produced when 2.00g of CS2 is burnt?
At stp what volume of SO2 gas will be produced when 2.00g of CS2 is burned
What volume of CO2 gas is produced when 20 gm of 20% pure CaCO3 is completely heated?
At 80.°C, Kc = 1.87 10-3 for the reaction. PH3BCl3(s) PH3(g) + BCl3(g) (a) Calculate the equilibrium concentrations of PH3 and BCl3 if a solid sample of PH3BCl3 is placed in a closed vessel at 80.°C and decomposes until equilibrium is reached. (b) If the
Hydrogen (H2) and oxygen (O2) combine to make water (H2O) in the following equation. 6H2 + 3O2 -> ?H2O How many water molecules would be produced? A. Six B. Four C. Three D. Five
Hydrogen (H2) and oxygen (O2) combine to make water (H2O) in the following equation. 6H2 + 3O2 → ?H2O How many water molecules would be produced? (1 point) five five three three six six four
Calcium carbonate of mass 10g was heated until there was no further change A. Write an equation for the reaction B. Calculate the mass of the residue C. Calculate the volume of gas evolved at STP D. What would be the volume of the gas measured at 15°C and
A hydrate of zinc nitrate has the formula Zn(NO3)2 . xH2O. If the mass of 1 mol of anhydrous zinc nitrate is 63.67% of the mass of 1 mol of the hydrate, what is the value of x?
Calculate the pH of a solution whose hydrogen ion concentration is 5×10^-9
Calculate the number of hydrogen atoms in 20.0 g of CH3OH
Please help me with this! What is the definition of a hydrocarbon? A) electrons shared between two different atoms B) a single line bonding carbon and hydrogen C) large molecules that are produced by living things D) a large chain of carbons and hydrogens
calculate the energies of the states of the hydrogen atom with n=2 and n=3, and calculate the wavelength of the photon emitted by the atom when an electron makes a transition between these two states.
When a diprotic acid, H2A, is titrated by NaOH, the protons on the diprotic acid are generally removed one at a time, resulting in a pH curve that has the following generic shape. (a) Notice that the plot has essentially two titration curves. If the first
Zinc fluoride (ZnF2) dissociates according to the following equation: ZnF2(s) ⇌ Zn2+(aq) + 2F–(aq) Ksp of this equilibrium is 3.0 × 10–2. If the concentration of zinc ions (Zn2+) in a solution is measured to be 4.4 × 10–1 M, what is the
Consider the following reaction. CH4(g) + 2 O2(g) CO2(g) + 2 H2O(l) ÄH = -891 kJ Calculate the enthalpy change for each of the following cases. (a) 5.00 g methane is burned in excess oxygen.
Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2H2O2(l) → 2H2O(l) + O2(g) ΔH = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.60 g of hydrogen peroxide decomposes at constant
Ammonia gas reacts with oxygen gas according to the following equation: 4NH3 + 5O2----4NO + 6H2O a. How many moles of oxygen gas are needed to react with 23 moles of ammonia? (29 mole) b. How may grams of NO are produced when 25 moles of oxygen gas react
The voltage generated by the zinc concentration cell (described by, Zn(s)|Zn2 (aq, 0.100 M)||Zn2 (aq, ? M)|Zn(s)) is 27.0 mV at 25 °C. Calculate the concentration of the Zn2 (aq) ion at the cathode.
A potassium permanganate solution containing 1.58 g of KMnO4 per liter is added into 5 ml of an acidified iron (||) sulfate solution .Decolorizing of KMnO4 solution ceases when 10ml of the solution has been added. Calculate the mass of FeSo4.7H2O which has
A 32.0 mL sample of hydrogen is collected over water at 20.0 degrees celcius and 750.0 torr. What is the volume of the dry gas at STP?
What volume of nitrogen dioxide (in L) is produced from the complete reaction of 16.87 of lead (ii) nitrate at STP
What is the volume of nitrogen that will be produced at stp from the decomposition of 9.60g of ammonium dioxonitrate(III)?
A compound containing only carbon, hydrogen and oxygen is subjected to elemental analysis. Upon complete combustion, a .1804g sample of the compound produced .3051g of CO2 and .1249g of H2O. What is the empirical formula of the compound?
When 1180 J of heat are added to one mole of an ideal monatomic gas, its temperature increases from 272 to 292 K. Find the work done by the gas during this process. I know the specific heat is Q/delta T, so C = (1180 J)/(20K) = 59. This seems like any easy
How many moles of water are produced when 1.05 g of oxygen gas reacts with 1.22 g of hydrogen gas to produce water?
Propane gas (C3H8) burns completely in the presence of oxygen gas (O2) to yield carbon dioxide gas (CO2) and water vapor (H2O). Write a balanced equation for this reaction. Assuming that all volume measurements occur at the same temperature and pressure,
What volume of 0.170 M K3PO4(aq) must be added to 50.3 mL of 0.103 M K2HPO4(aq) to prepare a buffer solution with a pH of 12.09?
Procedure: 1. Calculate the mass of iron(II) ammonium sulfate hexahydrate, Fe(NH©þ)©ü(SO©þ)©ü*6H©üO (MW = 392.14) required to make 100 mL of solution that is 0.2M in Fe©÷⁺ ions. You will be asked to show your calculation in the Assignment. 2.
Calculate the hydrogen ion concentration, pH, POH, OH‐ in 0.02 H2SO4?
C5H12 + O2--- CO2 + H2O give that the equation if I use 85 grams of O2 and excess C5H12 how many grams of CO2 are produced
Hydrogen gas can be produced by the reaction of magnesium metal with hydrochloric acid as shown in the following chemical reaction. Identify the limiting reagent when 6.00 grams of HCl reacts with 5.00 grams of Mg.
3.5g of CuCl2.2H2O were dissolved and reacted with excess Na2SO3 in the presence of HCl. After filtration, 1.5g of CuCl crystals was obtained. Calculate the %yield.
A copper Calorimeter of mass 150g,was half-filled with water of mass 300g and a temperature of 0°C.5g of ice of mass 0°C was added to the content, later some quantity of steam was passed into the mixture and the temperature rose by 20°C. Calculate the
What volume of 10.0 M NaOH is needed to prepare a buffer with a pH of 7.79 using 31.52 g of TrisHCl? ( Tris. At 25 ∘C, Tris has a pKb of 5.91 ) a) The buffer from Part A is diluted to 1.00 L. To half of it (500. mL), you add 0.0250 mol of hydrogen ions
What is the effect on the boiling point of a solution (for example, water) produced by a soluble nonvolatile substance (for example, sodium chloride)? What is the effect of an insoluble substance such as sand or charcoal? I believe if an insoluble
What volume of oxygen (at 82.1 oC and 713 mmHg) will be produced by the decomposition of 5.71 potassium chlorate? i am not sure what the unit is on the 5.71 ( cause it's not given) so that's not a typo.
how many moles of potassium carbonate will be produced if 400.0 g of potassium hydrogen carbonate are heated
Assuming that the volumes are additive, what volume of water must be added to 35.0mL of 23.0 M HCl to make a solution which is 3.00 M?
1. How much heat is released when 9.22 grams of glucose C6H12O6 reacts according to the following equation? C6H12O6 + 6O2 --> 6CO2 + 6H2O ∆H = -2803 kJ 2. How much heat is absorbed during photosynthesis when 9.22 grams of glucose C6H12O6 is produced?
Q5) The reaction for the combustion of propane is as follows: C3H8 + 5O2 ---->>3CO2 + 4H2O 1. If 20.0 g of C3H8 and 20.0 g of O2 are reacted, which is the limiting reactant? 2. How many grams of H2O can be produced? 3. How many grams of the excess reactant
Suppose 2 grams of an unknown metal carbonate MCO3 is reacted with excess HCl and 0.88 grams of CO2 are produced. What is the atomic mass (molar mass) of the unknown metal M? What element is it?
H2(g) + Cl2(g) HCl(g) Consider the unbalanced equation above. 3.95 L of H2 and 1.00 L of Cl2 are reacted under the same conditions of temperature and pressure. (a) How many liters of HCl will be produced? (b) How many liters of reactant are in excess? i
calculate the number of molecules in 6.4g of so2. (b) 1.5 moles of hydrogen chloride
Magnesium hydroxide is produced by reacting magnesium oxide with excess water. If the reaction has an expected yield of 81%, how much magnesium oxide should be reacted to produce 98.0 g of magnesium hydroxide? MgO(s)+H2O(l)->Mg(OH)2(aq)
In an experiment 4.0 g of ferrous ammonium sulphate, FeSO4.(NH4)2SO4.6H2O, is used. Since the oxalate in in excess, calculate the theoretical yield of the iron complex?
Hydrogen sulfide H2S is produced during decomposition of organic matter. when .5000 mol H2S burns to produce SO2 and H2O. -281.0 kJ of heat is released. what is this heat in kilocalories. Can you help me start this please
Nickel2 sulfate is produced when elemental nickel metal is dissolved in sulfuric acid to make nickel2 sulfate. Hydrogen gas is also released in the process. what is the balanced equation for this chemical reaction?
The combustion of 1.00g of vitamin C, compound that contains only carbon, hydrogen and oxygen produced 1.500g of co2 and 0.401g of H2O. Find the molecular formula of vitamin C knowing that its molecular mass is 176
Explain why a mixture of zinc oxide and magnesium reacts when heated while there is no reaction when a mixture of zinc and magnesium oxide is heated
A potassium hydroxide solution has a pH of 12.90. Enough cid is added to react with half of the OH- ions present. What is the pH of the resulting solution? Assume that the products of the neutralization have no effect on pH and that the amount of
1.A bus travels 400 m between two stops. It starts from rest and accelerates at 1.50 m/s^2 until it reaches a velocity of 9.00 m/s. The bus continues at this velocity and then decelerates at 2 m/s^2 until it comes to a halt. Find the total time required
The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated KHP). KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/mol. In the titration
Assume that the balloon is filled with carbon dioxide gas at 20°C and standard pressure. Use the ideal gas law to calculate the number of moles and mass of CO2 in each balloon at maximum inflation. balloon 1 volume-150.53 balloon 2 volume- 248.47 balloon
I had to perform an experiment for rate of reaction. The point of the experiment was to show how changes in reactant concentration, temperature, and catalyst presence can affect the rate of a reaction. The reaction that we studied was H2O2 + 2I^- + 2H^+ ->
Commercial vinegar usually has a concentration of 5%, per volume. a) Calculate the [H3O+] , if the density of acetic acid is 1.051 g/mL. b) Calculate the pH.
5)a. Electrons accelerated by a potential difference of 12.23 V pass through a gas of hydrogen atoms at room temperature. Calculate the wavelength of light emitted with the longest possible wavelength. b. Calculate the wavelength of light emitted with the
In the reaction N2 + 3H2 -> 2NH3, how many grams of NH3 gas would be formed when H2 gas, having a volume of 11.2 liters at STP, reacts with excess N2 gas? Completly confused, thank you very much for your help :)
For the reaction below, the equilibrium constant is Kc = 3.2×10−10 at 25 °C. Pb(s) + 2 Cr3+(aq) ⇌ Pb2+(aq) + 2 Cr2+(aq) Excess Pb(s) is added to a solution for which the initial concentration of Cr3+(aq) is 1.0 mol L−1. What are the equilibrium
N2 (g) + 3H2 (g) -> 2NH3 (g) assume 4 molecules of nitrogen and 9 molecules of hydrogen are present. after complete reaction, how many molecules of ammonia are produced. do i go from N to NH3 or H to NH3?
A 500 g piece of iron changes 7°C when heat is added. How much heat energy produced this change in temperature? C of iron is 0.450 J/g°C
In one experiment, the reaction of 1.00 g mercury and an excess of sulfur yielded 1.16 g of a sulfide of mercury as the sole product. In a second experiment, the same sulfide was produced in the reaction of 1.52g mercury and 1.02g sulfur. a) What mass of
9. when the [CO2] and [H2CO3] are both horizontal lines, the rate of the forward reaction is ____ The rate of the reverse reaction. a. faster then b. slower than c. The same as 10. if you added molecules of H2CO3 into the liquid, what do you think will
1)What is the longest wavelength light capable of ionizing a hydrogen atom in the n = 6 state 2)a. Calculate the energy of the electron in the ground state of single ionized helium, which has an atomic number Z = 2. b. Calculate the radius of its

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A solution of hydrogen peroxide, H2O2, is titrated with a solution of potassium permanganate, KMnO4. It requires 51.7 mL of 0.145 M KMnO4 to titrate 20.0 g of the solution of hydrogen peroxide. What is the mass percentage of H2O2 in the solution? If you
Aluminum reacts with sulfuric acid, which is the acid in automobile batteries. If 20.0 grams of Al is placed into a solution containing 115 grams of H2SO4, how many grams of hydrogen gas could be produced? Please help--I do not know how to set this one up.
What volume of water was added to the 350 mL of NaOH solution? Assume volumes are additive. Answer in units of mL
Nitric oxide (NO) reacts with molecular oxygen as follows: 2NO(g) + O2(g) �¨ 2NO2(g) Initially NO and O2 are separated as shown below. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end of the
Lab: Determining the Quantity of Vitamin C in Fruit Juice Vitamin C, also called ascorbic acid, is commonly found in commercial fruit juices and drinks. In this activity you will analyze data collected from a titration analysis of a fruit juice. The
Lab: Determining the Quantity of Vitamin C in Fruit Juice Vitamin C, also called ascorbic acid, is commonly found in commercial fruit juices and drinks. In this activity you will analyze data collected from a titration analysis of a fruit juice. The
Lab: Determining the Quantity of Vitamin C in Fruit Juice Vitamin C, also called ascorbic acid, is commonly found in commercial fruit juices and drinks. In this activity you will analyze data collected from a titration analysis of a fruit juice. The
Calculate ph value of soft drink having hydrogen ion concentration equal to 3x10^-5.
Calculate the mass of water having the same number of hydrogen atoms as are present in 32 gm of methane.
What volume of H2O should be added to 500 ML of a 1.0 mol/L CuSO4 solution to dilute it to 0.5 mol/L? This is what I have so far... H20 + CuSO4 --------> H2SO4 + CuO So you use the formula M1V1 = M2V2 so its (0.500)(1.0) = (0.5)(V) Solve for V, I got 1.0
Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s) + 2HCl(aq) --> ZnCl2(aq) + H2(g) When 0.114 g of Zn(s) is combined with enough HCl to make 51.1 mL of solution in a coffee-cup calorimeter, all of the zinc reacts,
In one process of 5.75 kg of CaF2 are treated with an excess of H2SO4 and yield 2.85 kg of Hf calculate the percent yield of hf?
Suppose that a firm is currently employing 20 workers, the only variable input, at a wage rate of $60. The average product of labor is 30, the last worker added 12 units to total output, and total fixed cost is $3,600. a. What is marginal cost? b. What is
1. To make a buffer using NH4OH, you must add a. a neutal salt b. you can't use it to make a buffer c. nothing d. its salt 2. Acidosis is a condition where the body fluids are too acidic. If someone with acidosis uses a lot of salt on their food, a. the
6CO2 + 6H2O → C6H12O6 + 4O2 How many molecules of carbon dioxide are involved in this reaction? How many molecules of sugar are produced in this reaction? How many atoms of carbon are on the left hand side of this equation? How many atoms of carbon are
Please help with this problem =) The combustion of liquid chloroethylene, C2H3Cl, yields carbon dioxide, steam, and hydrogen chloride gas. I. write a balanced equation for the reaction (I sorta get this part) II. How many moles of oxygen are required to
1. Engineers design air bags that deploy almost instantly upon impact. To do this, an air bag must provide a large amount of gas in a very short time. Many manufacturers use sodium azide, NaN3, to produce the gas in such a manner 2NaN3(s)  2Na(s) +
3Cu(s) + 8HNO3(aq) → 2NO(g) + 3Cu(NO3)2(aq) + 4H2O(l) If 15 g of copper metal was added to an aqueous solution containing 6.0 moles of HNO3, how many moles of NO(g) would be produced, assuming a 59.8 % yield.
Consider the titration of 40.0 mL 0.250 M ethylamine, C2H5NH2, with 0.350 M HCl. Determine each of the following and sketch the titration curve. Kb of ethylamine = 5.6x 10-4 a. The volume of added acid required to reach the equivalence point. b. The
A volume of 500.0 mL of 0.170 M NaOH is added to 595 mL of 0.200 M weak acid (𝐾a=6.74×10−5). What is the pH of the resulting buffer? HA(aq)+OH−(aq)⟶H2O(l)+A−(aq)
bornite(Cu3FeS3)is copper ore used in the production of copper.when heated,the following reaction occurs.2CuFeS3(s)+7oxygen(g)=6Cu(s)+2FeO(s)+6SO2(g)..IF 3.88 metric tons of bornite is reacted with excess oxygen and the process has 75.6 percent yield of
Need help solving this problem. A 0.188g sample of unknown metal, X (s), produced 71.4ml of hydrogen gas when reacted with HCl according to the equation: X(s)+2HCl(aq)--> XCl2(aq)+H2(g) The gas was collected over water at 23 degrees C. The levels of water
On complete oxidation, one mole of an organic compound produced four moles of water. Which one of the following substances could it be? CH4 C2H6 C3H7OH C4H10 So I added O2 to each of these compounds, but I must be doing something wrong because I can't get
PartA: What volume of 10.0M NaOH is needed to prepare a buffer with a pH of 7.79 using 31.52 g of TrisHCl? TrisHCl is a weak base and the molecular weight is 157.67 g/mol. I found the solution, it is 6.67 milliliters. The main question is:Part B: "The
Calculate the energy of a photon emitted when an electron in a hydrogen atom undergoes a transition from n = 6 to n = 1.
When excess solid Mg(OH)2 is shaken with 1.00 L of 1.2 M NH4Cl solution, the resulting saturated solution has pH = 9.30. Calculate the Ksp of Mg(OH)2 I am not sure where to even begin on this problem.
Determine the mass of copper(ii)trioxonitrate(v) that will be formed when 15grams of copper is added to excess dilute trioxonitrate(v).{cu=63.5,N=14,O=16} solution cu(No3)2=Cu N2 O6 =63.5+14x2+16x6 =63.5+28+96 =187.5 Number of mole=mass/molar mass
According to the following reaction, how many grams of iron(III) chloride will be formed upon the complete reaction of 27.1 grams of chlorine gas with excess iron? The balanced eq is 2Fe+3Cl2=2FeCl3 Here is my worked out equation: 27.1g Cl*1 mol Cl/35.46 g
Acettlene gas (C2H2) is used in welding. During one job, a welder burns 48.0 g of acetylene. Using a balanced equation for the complete combustion of acetylene, calculate the following: Balanced Equation a) the mass of oxygen used b) the mass if carbon
which statement best describes the types of bonds shown in the diagram? H CI = hydrogen chloride molecule 1. an ionic bond; the hydrogen ion is bonding with a chlorine atom. 2. an ionic bond; a hydrogen ion is bonding with a chlorine atom. 3. a covalent
Oxygen attracts electrons more strongly than hydrogen does. What kind of bond forms between the two hydrogen atoms and single oxygen atom that form a water molecule? A. A metallic bond B. A hydrogen bond C. An ionic bond D. A polar bond Currently stuck
Calculate whether or not a precipitate will form if 1.40 mL of 0.62 M NH3 are added to 4.4 L of 1.0 10-3 M FeSO4.
What is the increase in temperature necessary for a hydrogen gas, initially at 0°C, to increase its volume by 5% at constant pressure?
Calculate the number of moles of excess reactant that will be left-over when .350 g if HCN react with .500 g of 02: HCN+O2->N2+CO2+H20
Calculate the mass of each product formed when 43.82g of diborane (B2H6) reacts with excess water: B2H6(g) + H2O(l)--> H3BO3(s) + H2(g)
Calculate the number of moles of calcium chloride that can be obtained in 30g of calcium trioxocarbonate (vi) in the presence of excess hydrochloric acid
A buffer is created by mixing equal concentrations of NH4+ and NH3. Calculate the volume of both solutions needed to create a buffer of pH=8.75 with a total volume of 100 mL.
A certain volume of oxgen diffused from a given apparatus in 125 secs.In the same conditions,the same volume of gas N,diffuse in 100 secs.Calculate the relative molecular mass of N.
There is a current being applied to an aqueous solution fo sodium bromide. What is produced at the cathode and anode? I said that Na(s) being produced at the cathode and Br2(l) being produced at the anode. The other options are H2 and O2 for either but
When copper(II) oxide is heated in the presence of hydrogen gas, elemental copper and water are produced. What mass of copper can be obtained if 34.0 g copper(II) oxide is used?
Calculate the mass/volume percent of a NaCl solution in which 182g of NaCl is dissolved in enough water to give a total volume of 4.78L . Would I do 182/4780ml *100?
Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of sulfuric acid are needed to completely react with 15.0 mol of aluminum? 2Al(s) + 3H2SO4(aq) Al2(SO4)3(aq) + 3H2(g)
Calculate the heat released when 4.260 L Cl2 with a density of 2.46 g/L at 25°C reacts with an excess of sodium metal to form solid sodium chloride at 25°C.
The base JK of isosceles triangle HJK is produced to L.if J=69 calculate HKL
Can zinc (Zn) react with one of these: Al(NO3)3 aluminum nitrate Mg(NO3)2 magnesium nitrate Zn(NO3)2 zinc nitrate Cu(NO3)2 copper nitrate?
A 25.00mL sample of a household cleaning solution was diluted to 250.0mL in a volumetric flask. A 50.00mL aliquot of this solution required 40.38mL of 0.2506 M HCl to reach a bromocresol green end point. Calculate the weight/volume percentage of NH3 in the
Nitrobenzene, C6H5NO2, is prepared from benzene, C6H6, and nitric acid, HNO3. The other product of the reaction is water. When 22.4 g of benzene is reacted with an excess of nitric acid, 31.6 g of nitrobenzene is produced. What is the percent yield for
what will volume of ammonia gas when 100cm^3of nitrogen reacts with 150cm^3of hydrogen?which is the limiting reactant?
When hydrogen peroxide (H2O2) is used in rocket fuels, it produces water, oxygen, and heat. 2H2O2(l)⟶2H2O(l)+O2(g)ΔH=−196kJ How many kilojoules are released when 2.65 moles of H2O2 reacts? How many kilojoules are released when 234 g of O2 is produced?
In the titration of 50.0 mL of 1.0 M CH3NH2 (kb=4.4 x 10^-4), with 0.50 M HCl, calculate the pH a) after 50.0 mL of 0.50 M has been added b) at the stoichiometric point.
Calculate the number of moles of hcl(aq)added to sodium thiosulphate
if 8.100 grams of C6H6 is burned and heat is produced from the burning is added to 5691 grams of water at 21 degrees celsius what is the final temp of the water? 2C6H6+15O2=12CO2+6H2O+6524kj
Barium sulfate forms as a precipitate in the following reaction: Ba(NO3)2 (aq) + Na2SO4 (aq) -> BaSO4 (s) + 2NaNo3 (aq) When 35.0g of Ba(nO3)s is reacted with excess Na2SO4, 29.8g of BaSO4 is recovered by the chemist. a) Calculate the theoretical yield of
1) How many drops of 12M HCl would you add to 1.00 L of 0.100 M HC2H3O2 to make [C2H3O2-] = 1.0 x 10^-4 M? Assume that 1 drop = 0.050 mL and that the volume of the solution remains 1.00 L after the 12 M HCl is diluted. [Hint: What must be the [H3O+] in the
Calculate the number of mole of cacl2 calcium chloride that can be obtained frm 30g of calcium trioxocarbonate iv in the presence of excess hydrochloride acid
A mixture of 3.00 volumes of H2 and 1.00 volume of N2 reacts at 344 C to form ammonia. The equilibrium mixture at 110.0 atm contains 47.00 % NH3 by volume. Calculate Kp for the reaction, assuming that the gases behave ideally.
A sample of peanut oil weighing 2g is added to 25ml of 0.4M koh. After saponification is complete, 8.5ml of 0.28M hes04 is needed to neutralize excess of koh. The saponification number of peanut oil. The right answer 146.75 Bob solve it for me step by step
Calculate the molar entropy of vaporization for liquid hydrogen iodide at its boiling point, �34.55°C. HI(l)7HI(g) �Hvap � 19.76 kJ/mo
Calculate the hydrogen ion concentration and the pH of each of the following solutions of strong acids. (a) 0.00010 M HCl if you could just explain how to do this that would be great! thanks
calculate the wavelength of the second line in the Brackett series (nf=4) of the hydrogen emission spectrum. Rh= 2.180e-18 any help please? i know its energy levels 4 to 6... but that is all.
The following equilibrium was studied by analyzing the equilibrium mixture for the amount of H2S produced. Sb2S3(solid)+3H2(gas)2Sb(solid)+3H2S(solid) A vessel whose volume is 2.5L is filled with 0.0100 mole of antimony(III)Sulfide, Sb2S3, and 0.0100 mole
I have .8ml of 35% by weight hydrogen peroxide. The hydrogen peroxide density is 1.14 g/ml. how many moles of hydrogen peroxide are there?
The overall cell reaction occurring in an alkaline battery is: Zn(s) + MnO2(s) + H2O(l) ---> ZnO(s) + Mn(OH)2(s) a) How many moles of electrons flow per mole of reaction?...answer: 2. Mol e-Note: b) If 6.09g of zinc is oxidized, how many grams of manganese
Acetic acid ionizes in water as follows: CH3COOH + H2O CH3COO– + H3O+ Fewer than 1% of ethanoic acid molecules are ionized at any instant. The acetate ion (CH3COO– ) is therefore ____. A.a poor hydrogen-ion acceptor B.a good hydrogen-ion acceptor C.a
if 7.5g of urea, (NH2)2CO is dissolved in 500g of water (density of resulting solution is 1.25g/mml). what is the molar concentration of the solution?
Hydrogen reacts w/ sodium to produce solid sodium hydride, NaH. A reaction mixture contains 6.75 g Na and 3.03 g H2. A. Which reactant is limiting? B. What is the theoretical yield of NaH from the above reaction mixture? C. What is the percent yield if 4 g
What volume (in mL) of an 8% w/v acetic acid solution would be needed to form 2.2 L of carbon dioxide gas at 25.2 degrees Celsius and 0.9982 atm? Assume the acid is reacted with excess sodium bicarbonate, and round your final answer to two sig figs.
if electricity of sufficient voltage is passed into a solution of potassium iodide in water, a reaction takes place in which elemental hydrogen gas and elemental iodine are produced, leaving a solution of potassium hydroxide. what is the unbalanced
NH3 is normally encountered as a gas with a pungent odor. It is formed from hydrogen and nitrogen (equation given below). A chemist pours a mixture of nitrogen gas and hydrogen gas in a 1.0 litre reaction vessel in 1:3 ratio. The equilibrium constant
What is the total volume of gases produced at 819 K and 1. atm pressure when 320 g of ammonium nitrite undergoes the following decomposition reaction? NH4NO2 --------> N2(g) + 2H2O(g)
Treatment of a 0.2500-g sample of impure potassium chloride with an excess of AgNO3 resulted in the for- mation of 0.2912 g of AgCl. Calculate the percentage of KCl in the sample.
determine the volume of the residual gas at 20.0cm³ of hydrogen was sparked with 15.0cm³ of oxygen and the resulting mixture cooled at room temperature
a) Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH)2. b) A 0.850-mole sample of nitrous oxide, a gas used as an anesthetic by dentists, has a volume of 20.46 L at 123°C and 1.35 atm. What would be its volume at 468°C and
Calculate the theoretical yield of alum if 0.200g of Aluminum was reacted with excess KOH and H2SO4? I don't even know how to start it. Please help. Also I wanted to say thank you for the help I've gotten from this website it has helped me a lot. I feel
1. How do plants recycle carbon during photosynthesis?(1 point) The carbon in carbon gas is recycled as glucose.**** The carbon in glucose is recycled as carbon gas. The carbon in carbon dioxide is recycled as glucose. The carbon in glucose is recycled as
What is the pH of a solution having a hydrogen ion concentration of 1x10^-5 M? Also the same question, but Hydroxide instead of hydrogen. thanks in advance!
Find the volume of the solid generated by revolving the region bounded by the given lines and curves about the y-axis: y=(x-2)^3-2, x=0, y=25 Solve by either the disk or washer method. I calculated the volume using the shell method and got 1250pi. However,
A student collected H2 gas in a buret by displacing water at 22.0 °C. The buret could not be submerged deep enough in a water bath to equalize the pressure. The water level in the buret was 18.2 cm above the water level in the water bath. The volume of
calculate the max wavelength of light capable of removing an electron for a hydrogen atom from the energy state characterized by the following : n=2 in nm n=4 in nm
Calculate the wavelength of light that must be absorbed by hydrogen atom in its ground state to reach the excited ste of E=+2.914*10^(-18)
calculate the percent yield of Cl2 in the electrolytic decomposition of hydrogen chloride if 25 g of HCl produces 13.6 of chlorine gas.
A certain volume of co2 take 200 sec to diffuse through a porous plug how long eill it take the same volumeof hydrogen chloride gas to diffuse under same condition
1.0 g of hydrogen reacts completely with 19.0 g of fluorine. What is the percent by mass of hydrogen in the compound that is formed? My answer: 5.2631578947368
Many homes in rural America are heated by propane gas, a compound that contains only carbon and hydrogen. Complete combustion of of a sample of propane produced 2.641 grams of carbon dioxide and 1.422 grams of water as the only products. Find the empirical
Calculate the amount of water produced by the combustion of 44g of propane and 16g of methane.
the base JK of isosceles triangle HJK is produced to L. if J equals 69 degree, calculate HKL
Calculate the extension that would be produced by a 20N force if 15N extends a spring by 3cm
calculate the number of gram of Al2S3 which can be prepared by the reaction of 20 gram of Al and 30 gram of sulpher . how much the non limiting reactant is in excess?
NH3 is normally encountered as a gas with a pungent odor. It is formed from hydrogen and nitrogen (equation given below). A chemist pours a mixture of nitrogen gas and hydrogen gas in a 1.0 litre reaction vessel in 1:3 ratio. The equilibrium constant
I'm doing a redox potential/lead acid cell experiment and one of the questions that were asked was: -What were the identities of the gases you saw being produced at the + and - electrodes during the cell conditioning process? We used H2SO4 How do I go
CH3NH2(aq)+H2O(l)=>CH3NH3+(aq)+OH-(aq) Kb=4.4 x 10^-4 Methylamine, CH3NH2, is a weak base that reacts with water according to the equation above. A student obtains a 50.0 mL sample of a methylamine solution and determines the pH of the solution to be
CH3NH2(aq)+H2O(l)=>CH3NH3+(aq)+OH-(aq) Kb=4.4 x 10^-4 Methylamine, CH3NH2, is a weak base that reacts with water according to the equation above. A student obtains a 50.0 mL sample of a methylamine solution and determines the pH of the solution to be
Some hydrogen gas is enclosed within a chamber being held at 200C with a volume of 0.025m^3. The chamber is fitted with a movable piston. Initially, the pressure in the gas is 1.50*10^6 Pa (14.8 atm). The piston is slowly extracted until the pressure in
Q - An electrochemical reaction occurs between an unknown element and zinc. The half-cell reaction for the zinc is: Zn(s) → Zn2+(aq) + 2e− The cell potential for the reaction is Eºcell = 1.83 V. Is the reaction spontaneous or nonspontaneous? Explain.
if you're given a chart of half cell potentials (reduction potentials), how can you figure out which metals produce the highest voltage? For ex. Cadmium (Cd) with copper (Cu) Silver (Ag) with zinc (Zn) Lead (Pb) with zinc (Zn) would you say that pb and zn
A student titrated 1.852 g of a mixture containing potassium hydrogen phthalate, KHP....? A student titrated 1.852 g of a mixture containing potassium hydrogen phthalate, KHP, with 0.163 M NaOH solution. She recorded an initial buret reading of 0.84 mL and
a box with a volume of 22.4 L CONTAINS 1.0 mol of nitrogen and 2.0 mol of hydrogen at zero degrees celcius. Which of the flollowing statements is true? the correct statement is the partial pressure of N2 is 101kPa. How come??
Using data from the following reactions and applying Hess's law, calculate the heat change for the slow reaction of zinc with water (answer must be in kJ/mol Zn): Zn(s) + 2 H2O(l) ----> Zn^2+(aq) + 2 OH-(aq) + H2(g) (ΔHrxn = ?) H+(aq) + OH-(aq) ---->
Using a table of standard electrode potentials (such as the one in your textbook), calculate the standard cell potential for a cell made by placing a zinc electrode in a Zn2+(aq) solution which is connected by an electrolyte to a Ag+ (aq) solution
Calculate the molar entropy of vaporization for liquid hydrogen iodide at its boiling point -34.55 degrees celcius. HI(l) HI(g) deltaHvap = 19.76 kJ/mol

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1.Calculate the volume occupied by 3.2g of oxygen at 300K and 100KNm^-2.(R=8.3J/mol/K,Oxygen =16). 2.Calculate the volume occupied by 0.125mol of Oxygen at 27°C and a pressure of 2.02×10^5Nm^2.(1mole of gas occupies 22.4dm^3 at Standard temperature and
A zinc-copper battery is constructed as follows (standard reduction potentials given below): Zn | Zn2+ (0.10 M) || Cu2+ (2.50 M) | Cu Zn2+ + 2 e- → Zn(s) Eº = -0.76 V Cu2+ + 2 e- → Cu(s) Eº = 0.34 V The mass of each electrode is 200 g. Each half-cell
Light from three different lasers (A, B, and C), each with a different wavelength, was shined onto the same metal surface. Laser A produced no photoelectrons. Lasers C and B both produced photoelectrons, but the photoelectrons produced by laser C had a
The density of hydrogen at STP is 0.09 g/l what is the mass of the sample of hydrogen.
Copper reacts with nitric acid according to the following reaction: 3 Cu (s) + 8 HNO3 (aq) --> 3 Cu(NO3)2 (aq) + 2 NO (g) + 4 H2O (l) If an pre 1982 copper penny contains 3.10 grams of copper, what volume of 8.00 M nitric acid is required to exactly
Calculate no: of moles of cl2 produced at equilibrium when 1 mole of pcl5 is heated in 10 DM vessel kc 0.041
Calculate the torque produced by a force of 50.0 N applied clockwise perpendicular to the end of a bar of length 0.50 m.
a 50.0 ml sample of a 15% (m/v) solution of H2SO4 is added to water to give a final volume of 250.0 ml. What would the final concentration be?
When one mole of C6H6 is burned, 3.27 MJ of heat is produced. When the heat from burning 7.47 g of C6H6 is added to 5.69 kg of water at 21.0°C, what is the final temperature of the water?
What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M aluminum nitrate is added to 200.0 mL of 0.100M potassium hydroxide?
Bornite (Cu3FeS3) is a copper ore used in the production of copper. When heated, the following reaction occurs. 2 Cu3FeS3(s) + 7 O2(g) 6 Cu(s) + 2 FeO(s) + 6 SO2(g) If 3.88 metric tons of bornite is reacted with excess O2 and the process has an 75.6% yield
How do plants recycle carbon during photosynthesis?(1 point) The carbon in carbon dioxide is recycled as glucose. The carbon in glucose is recycled as carbon gas. The carbon in carbon gas is recycled as glucose. The carbon in glucose is recycled as carbon
if 465cm Of Sulphur Oxide (So2) Can Diffuse Through Povous Portition In 30secs How LONg Will Equal Volume, 620cm^3 Of Hydrogen Sulphide (H2S) TaKe To Diffuse Through The Same Partition H 1, S 32, O 16
When hydrochloric acid reacts with sodium sulfide, hydrogen sulfide gas and sodium chloride are produced. How many moles of H2S will be generated by 2.56 moles of HCl? 2HCl + Na2S → H2S + 2NaCl
100. mL of 0.020 M CaCl2(aq) is added to 200. mL of 0.20 M K2SO4(aq). Calculate the equilibrium concentrations of Ca^2+ (aq) and SO4^2-(aq)
What volume of 3.0M Na2SO4 must be added to 25ml of 1.0M BaCl2 to produce 5.0g of BaSO4? The answer is 7.1ml but I don't get it very well. I thought I could use mole ratio of the balanced equation, but it did not work. Thanks a lot!
A factory produced 2300 TV sets in its first year of production. 4500 sets were produced in its second year and 500 more sets were produced in its third year than in its second year. How many TV sets were produced in three years?
A solution of Na2CO3 is added dropwise to a solution that contains 1.34×10−2M Fe^2+ and 1.33×10−2M Cd^2+ . What CO3^2- concentration of is need to initiate precipitation? Neglect any volume changes during the addition.
A 5 mL sample of 50% (m/v) acetic acid (Hc2H3O2) solution is added to water to give a final volume of 25 mL....what is the final concentration?
What is the pH change of a 0.220M solution of citric acid (pKa=4.77) if citrate is added to a concentration of 0.155M with no change in volume?
The molecular mass of glucose is 180g/mol. you prepare a stock solution of glucose, by dissolving 1.8g of glucose in water to a final volume of 1.0L. The stock solution was then diluted as follows: a. 50mL of the stock solution is added to 450mL of water,
Using Table 9.4, calculate an approximate enthalpy (in kJ) for the reaction of 1.02 g gaseous methanol (CH3OH) in excess molecular oxygen to form gaseous carbon dioxide and gaseous water.
An unknown volume of water at 18.2 degrees celsius is added to 24.4 mL of water at 35.0 degrees celsius. If the final temperature is 23.5 degrees celsius what was the unknown volume? (assume no heat is lost to surroundings and D of water is 1.00g/mL)
Use Rydbuz equation to calculate the wavelength of the third line in the paschen series of the hydrogen spectrum.give ur answer in Nm. RH=2.18 * 10^-18j, H=6.63 * 10^-34J. Plz help m
The diameter of a hydrogen nucleus is 1.0 X 10 -3 pm and its mass is 1.67 X 10 -24 g. What is the density of the nucleus in grams per cubic centimeter? Assume the nucleus is a sphere with volume = 4/3pie r3.
3. An electrochemical reaction occurs between an unknown element and zinc. The half-cell reaction for the zinc is: Zn(s) → Zn2+(aq) + 2e− The cell potential for the reaction is Eºcell = 1.83 V. a. Is the reaction spontaneous or nonspontaneous?
A certain volume of oxygen diffused from a given apparatus in 125 seconds. In the same conditions , the same volume of gas N, diffused in 100 seconds . Calculate the relative molecular mass of N(=16.0).
A gas-filled balloon having a volume of 1.50 L at 1.2 atm and 25°C is allowed to rise to the stratosphere (about 30 km above the surface of Earth), where the temperature and pressure are -23°C and 3.00 multiplied by 10-3 atm, respectively. Calculate the
1)A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared. Calculate the initial pH of this solution. The Ka for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. *A buffered solution resists a change in pH.*
We used a buret today, and I don't get how to calculate volume. I have an initial reading of 49.97 and a final buret reading of 30.49. How do I get the volume? I thought I just subtracted the final from the initial, but someone said their tutor told them
If a current of 5.0 Amps is passed through the electrolytic cell for .5 hour, how should you calculate the number of grams of bromine produced?
Calculate how many milliliters of carbon dioxide would be produced theoretically from 2.0g of sucrose at 25 deg Cel and 1 atm pressure.
Need help with this lab: (sorry so long) Hypothesis: The amount of product will be regulated by the limiting reactant. Procedure: First, I took two test tubes from the Glassware shelf. I added 6 mL of the copper sulfate solution to one, and 6 mL of the
A chemist must dilute of M aqueous magnesium fluoride solution until the concentration falls to M . He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in liters
Standardization of the Sodium Thiosulfate Solution Make up a standard solution of potassium iodate by accurately “weighing by difference” about 0.1 g of KIO3 and placing it in your 100 mL volumetric flask. Fill the flask to mark with distilled water.
An unknown compound, X, is though to have a carboxyl group with a pKa of 2.0 and another ionizable group with a pKa between 5 and 8. When 75 mL of 0.1M NaOH is added to 100 mL of a 0.1M solution of X at pH 2.0, the pH increases to 6.72. Calculate the pKa
What volume (in milliliters) of 0.180 M NaOH should be added to a 0.135 L solution of 0.0230 M glycine hydrochloride (pKa1 = 2.350, pKa2 = 9.778) to adjust the pH to 2.73? Plz help, I'm not sure how to answer the question! Thank you!!
Calculate the mass of solid AgNo3 that can be added to 2.0 L of 0.10M K2CrO4 solution in order to just start precipitation?
Volume of nitrogen gas is 125ml atmospheric pressure is 763mm Hg the water temperature inside the eudiometer is the same as the level of the water in the beaker. Calculate the volume if the nitrogen at STP. P1V1/T1=P2V2/T2
When 2.25 g of sodium hydroxide (NaOH) was dissolved in 150.00 g of water a value of 11.00oC was obtained for ΔT. 1. Calculate the molarity of the sodium hydroxide solution. 2. Calculate the value (calories) for the heat of solution of 2.25 g of NaOH. 3.
Hydrogen peroxide can be prepared in several ways. One method is the reaction between hydrogen and oxygen, another method is the reaction between water and oxygen. Calculate the ΔG°rxn of each reaction below? 1) H2(g) + O2(g) H2O2(l) ΔG°rxn=? (in kJ)
4. Vitamin C, M= 176.12 g/mol, is a compound of composed of carbon, hydrogen, and oxygen. Vitamin C is found in many natural sources especially citrus fruits. When a 1.000-g sample of vitamin C is burned in a combustion apparatus 1.50 g of CO2 and 0.410 g
"Given: An aqueous solution of C6H12O6 with a density of 1.18 g/ml" I) Calculate Molarity 1) It firsts asks me to, "State the moles of solute" 2) Calculate the mass of the solute in grams - I think I can do this if I know how to get #1 3) Later it also
What volume of 0.149 M HCl must be added to 1.00x10^2 mL of 0.285 M HCl so that the resulting solution has a molarity of 0.205 M? Assume that the volumes are additive.
What volume of WATER MUST BE ADDED to 10.0 mL of 6.0 M NaOH to make a solution that is 0.30 M in NaOH? Assume that the volumes are additive. a. 10 mL b. 190 mL c. 200 mL d. 210 mL e. 500 mL
The mass of a dry, 50 mL beaker is 49.135 g. The observed volume of water in a volumetric pipet is 20.00 mL. This water is transferred to the beaker and the combined mass of the water and the beaker is found to be 69.122 g. Given that the density of water
A mixture of nitrogen gas and hydrogen gas reacts in a closed container to form ammonia gas. The reaction ceases before either reactant is completely consumed. At this stage the container has 3.0 mol each of all three gases; nitrogen, hydrogen and ammonia.
4NH3 + 5O2 → 4NO + 6H2O 2NO + O2 → 2NO2 3NO2 + H2O → 2HNO3 + NO In this process, the NO made in the last reaction is recycled back into the second reaction and used as a reactant. In the end, all of the NO produced is recycled back so that when the
A container is charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H2(g) + N2(g) 2 NH3(g)
Calculate the hydrogen ion concentration, in moles per liter, for solutions with each of the following pH values. pH=1.10 im guessing that this is what i did in my previous question except now i have to do it backwards. but i don't know how to do the
In an experiment to determine the solubility of lead chloride (PbCl2), 5.6g of (NH4)2SO4 was added to a 250ml solution containing an unknown amount of dissolved lead chloride (PbCl2) resulting in the formation of Lead sulfate precipitate. The mass of the
Ammonia is not the only possible fertilizer. Others include urea, which can be produced by the reaction, CO2(g) + 2 NH3(g) --> CO(NH2)2 (s) + H2O(g). A scientist has 75g of dry ice to provide the carbon dioxide. If 4.50L of ammonia at 15C and a pressure of
treatment of a 0.400g sample of impure potassium chloride with an excess of AgNO3 resulted in the formation of 0.733g of AgCl. calculate the percentage of KCl in the sample. show balanced equations in support of your answer
can you calculate the mass(g) of AL2O3 that is produced when 2.5g of aluminum and 2.5g of oxygen react according to this equation : 4Al(s)+3O2(g)->2Al2O3(s) im not understanding how to do this
A mixture contains only NaCl and Al2(SO4)3. A 1.45-g sample of the mixture is dissolved in water and an excess of NaOH is added, producing a precipitate of Al(OH)3. The precipitate is filtered, dried, and weighed. The mass of the precipitate is 0.107 g.
calculate the mass of solid NaCl that must be added to 1.5L of 0.100M AgNO3 solution to precipitate all the Ag+ ions in the form of AgCl?
2SO2(g) + O2(g) >2SO3(g). If 96g SO2 is added to 2 moles of oxygen at STP, calculate the mass of SO3 that is formed
A 30.00mL sample of 0.150M KOH is titrated with 0.125M HClO4 solution. Calculate the pH after the following volumes of acid have been added: 30.0 mL, 35.0 mL, 36.0 mL, 37.0 mL, 40.0 mL
When 1.00 g. of MgCO3 is added to 2.0 L of water, some, but not all, will dissolve to form a saturated solution. Calculate the mass of solid that remains undissolved.
Please double check one last time have to hand it in tomorrow.Thank-You in Advance. This was the lab experiment: ------------------------------------------- A. Standardization of the Sodium Thiosulfate Solution Make up a standard solution of potassium
was hoping someone can help me check if these answers make sense for a silver copper alloy lab. 3. Why don’t you have to weigh the sodium chloride on a sensitive balance? This one I am not sure about, It is because an excess of NaCl is needed to make
1. How does hydrogen fuel cell work Chemical reaction within a hydrogen fuel cell convert hydrogen to gasoline, which can be used to power the car Chemical reactions within a hydrogen fuel cell produce electricity, which can be used to power an electric
If 10.5 g of hydrogen, H2, were mixed with 6.51 g of acetylene, C2H2, and allowed to react according to the following equation, what is the theoretical yield of ethane,C2H6 produced? If 7.00g of ethane, C2H6 were recovered at the end of the reaction , what
Aluminum reacts with sulfuric acid, which is the acid in car batteries. If 20.0 grams of Al is placed into a solution contain 115 gram of H2SO4, how many grams of hydrogen ga could be be produced? 2Al + 3H2SO4 ---> Al(SO4)3 + 3H2 20.0g/27 = .741 .741 X 3/2
A 0.450-gram sample of impure CaCO3(s) is dissolved in 50.0 mL of 0.150 M HCl(aq). The equation for the reaction is: CaCO3(s)+2HCl(aq) -> CaCl2(aq) + H2O(l) + CO2(g) The excess HCl(aq) is titrated by 9.75 mL of 0.125 M NaOH(aq). Calculate the mass
25g of NH3 is mixed with 4 moles of O2 in given reaction. 4NH3(g)+5O2(g)-->4NO(g)+6H2O(1)
One possible energy source for the mysterious object you've just discovered is the fusion of hydrogen to form carbon-12 (the most common and stable isotope of Carbon). Hydrogen has an atomic mass of 1.00794 u, while carbon has an atomic mass of 12.010 u.
What volume, in millilitres, of distilled water must be added to 105 mL of 0.600 mol/L sulfuric acid solution in order to dilute it to a concentration of 0.400 mol/L
When the electron in a hydrogen atom moves from n = 5 to n = 1, light is emitted. Calculate the energy of the light?
7. Calculate the density of hydrogen sulfide, H2S, at 56 ºC and 967 mmHg. (Express density in g/L)
(a) Use Boyle's law to calculate the volume the gas will occupy if the pressure is increased to 1.79 atm while the temperature is held constant. 3.17 L (b) Use Charles's law to calculate the volume the gas will occupy if the temperature is increased to
Hi everyone, I have been trying to figure out this titration equation all day and for some reason I am stumped. Here is the question in full: Potassium hydrogen phthalate, KHP, can be obtained in high purity and is used to determine the concentrations of
Calculate how many moles of products(s) would be produced if 0.500 mole of the first reactant were to react completely. BaCl2 + 2AgNO3 --> 2AgCl +Ba(NO3)2
Calculate the mass of O2 produced of 3.450g potassium chlorate is completely decolmposed by heating in the presence of a catalyst (Magnese dioxide).
A compound contains only carbon, hydrogen, nitrogen, and oxygen. Combustion of 0.157 of the compound produced 0.213g CO2 and 0.0310 g H20. In another experiment, it is found that 0.103g of the compound produces 0.0230 g NH3. What is the empirical formula
a 500ml stock solution of NAOH has a purity of 70% and a density of 1.9g/ml. calculate the concentration that would be in a 1L solution. calculate the molarity. What volume would we have to take to prepare 250ml of a solution of 0.1 mol/l
60cm3 of hydrogen diffused through a porous membrane in 10minutes.The same volume of gas G diffused through the same membrane in 37.4 minutes .Determine the relative molecular mass of G.(H=1)
A little red wagon with mass 7.0kg moves in a straight line on a frictionless horizontal surface. It has an initial speed of4.00 m/s and then is pushed 3.0m in the direction of the initial velocity by a force with a magnitude of 10.0 N a.) Use the
When 0.250 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical equation shown below, 177 kJ of heat are released. Calculate the value of Delta H for this reaction, as written. 2CH4(g)+3Cl2(g)-->2CHCl3(l)+3H2(g) delta H=?
1) Using the 1st equivalence point from part a calculate the molarity of the phosphoric acid. Molarity of NaOH = .1523 M Volume of phosphoric acid used 10.0mL Volume at equivalence point 7.410 mL and 14.861 mL 2) Using the 2nd equivalence point from part
The voltage generated by the zinc concentration cell described by, Zn(s)|Zn2+ (aq, 0.100 M)||Zn2+ (aq, ____ M)|Zn(s) is 24.0 mV at 25 °C. Calculate the concentration of the Zn2 (aq) ion at the cathode. Hi, I posted this question awhile back but I think it
Calculate the pressures, P, in atmospheres at which the mean free path, l, of a hydrogen molecule will be 1.50 μm, 1.50 mm, and 1.50 m at 20.0 °C. The diameter of a H2 molecule is 270 pm. Which formula would I use?
A GLASS CUP OF ORANGE JUICE IS FOUND TO HAVE A POH OF 11.40. CALCULATE THE CONCENTRATION OF THE HYDROGEN ION IN THE JUICE.
A glass cup of orange juice is found to be POH of 11•40. Calculate the concentration of hydrogen ion in the juice?
Arrange the three metals(Cu, Zn, and Mg) in order of their relative strengths as reducing agents, placing the strongest first. Arrange the three metallic ions ( Cu(No3)2, Zn(No3)2, and Mg(No3)2 ) in order of their relative strengths as oxidizing agents,
A gas at 250K and 15atm has a molar volume smaller than calculated from perfect gas law Calculate: a) the compression factor under these conditions b) the molar volume of gas
If 465 cm³ of sulphur(IV)oxide,can be diffuse through porous partition in 30s how long will(a) an equal volume , (b)620cm³ of hydrogen sulphide take to diffuse through the same partition ?(H=1,S=32,O=16)
I don't understand how to even start this problem: A mixture of H2(g), O2(g), and 2 mL of H2O is present in a 0.5 L rigid container at 25 degrees Celsius. The number of moles of H2 and the number of moles of O2 are equal. The total pressure is 1146 mmHg.
what mass of 25% ba(n03)2 solution contain 40 grams of ba(n03)2 ? Answer 160g My calculation 40g/261.37g/mol = 0.15305/0.25g = 0.612 This answer is not right Who helps
Write a piecewise definition for the tax due T(x) on an income of x dollars When x
what volume of 0.120 M NaOH must be added to 100 ml of 0.100 M NaHC2O4 to reach ph of 4.70? H2C2O4 Ka1 = 5.9 x 10-2 HC2O4^- Ka2 = 5.1 x 10-5 The answer is 60 ml but I don't know how to find it. Can you please show me the steps and how to do it please
A chemist must dilute 55.6 ml of 1.48 M aqueous silver nitrate (AgNO3) solution until the concentration falls to 1.00M. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in
If 10.00 g of water are introduced into an evacuated flask of volume 2.500 L at 65 degreed celcius, calculate the mass of water vaporized. (Hint: Assume that the volume of the remaining liquid water is negligible; the vapor pressure of water at 65 degrees
Lab: Determining Ka of Acetic Acid Purpose: The purpose of this experiment is to determine the molar concentration of a sample of acetic acid and to calculate its Ka. Materials: phenolphthalein 125 mL Erlenmeyer flask 25 mL pipet and bulb pH metre acetic
In the first 14.0 s of the reaction, 1.7×10−2 mol of O2 is produced in a reaction vessel with a volume of 0.340 L What is the average rate of the reaction over this time interval? 2 N2O(g) → 2 N2(g)+O2(g)
A glass in the form of a frustum of a cone is represented by the diagram below. The glass contains water to height of 9 cm. The bottom of the glass is circle of radius 2cm while the surface of the water is a circle of radius 6 cm. (a) Calculate the volume
Need Help with these two problems 1.One piece of copper jewelry at 111°C has exactly twice the mass of another piece, which is at 36.0°C. Both pieces are placed inside a calorimeter whose heat capacity is negligible. What is the final temperature inside
Assuming titration was carried out between sodium hydrogen tetraoxosulphate (vi)(NaHSo) of concentration 12.0gdm-² as solution A and 25cm³ of sodium hydroxide(NaOH) as solution B What is the volume of the pipette used ?
Hydrogen iodide can decompose into hydrogen and iodine gases. 2HI(g) mc026-1.jpg H2(g) + I2(g) K for the reaction is 0.016. If 0.148 atm of HI(g) is sealed in a flask, what is the pressure of each gas when equilibrium is established?
Iron pyrite (FeS2) is the form in whichmuch of the sulfur exists in coal. In the combustion of coal, oxygen reacts with iron pyrite to produce iron(III) oxide and sulfur dioxide, which is a major source of air pollution and a substantial contributor to

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A liquid solution of formaldehyde is 37% pure. This solution has a specific gravity of 1.037. The molecular weight of formaldehyde is 30.0. To 1.00 ml of this impure stock solution is added quantity sufficient total the total volume to 500 ml. If 1.00 ml
Determine the molarity of a 15.0 % by mass Hydrogen Peroxide solution. The density of Hydrogen Peroxide is 1.054 g/mL. The 15.0% by mass can be broken apart into 15.0 g Hydrogen Peroxide and 100.0 g solution. Use the density of Hydrogen Peroxide solution
Lysine is a compound composed of carbon, hydrogen, nitrogen and oxygen. When 1.50 g of lysine is burned, 2.72 g of carbon dioxide, 1.29 g of water and 0.287 g of nitrogen gas are produced. What is the empirical formula of lysine? If the molar mass of
Complete combustion of a sample of propane produced 2.641g of carbon dioxide and 1.442g of water as the only products. Find the empirical formula of propane. I have already calculated the number of moles for both water and carbon dioxide. I also know that
An oil droplet with a mass of 3.50 x 10^-15 kg accelerates downward at a rate of 2.50 m/s2 when it is between two horizontal charged plates that are 1.00 cm apart. Assuming that the excess charge on the droplet is negative and the top plate is positive,
a rigid vessel of volume 1m(^3) contains steam at 20bar and 400 degrees Celcius. The vessel is cooled until the steam is just dry saturated. Calculate the mass of steam in the vessel, the final pressure of the steam and the heat rejected during the
use the table below to calculate ΔHo reaction: Standard Enthalpies of Formation, ΔH˚fٍ at 298 K Substance - Formula - ΔH˚ƒ(kj/mol) Acetylene C2H2(g) 226.7 Ammonia NH3(g) -46.19 Benzene C6H6(l) 49.04 Calcium Carbonate CaCO2(s) -1027.1 Calcium Oxide
What effect does doubling the radius of a cylinder have on the volume of the cylinder? A. The volume is doubled. B. The volume is quadrupled. C. The volume is halved.*** D. The volume is multiplied by one-fourth. Im not sure what the answer is so If you do
A .682 g sample of an unknown weak monoprotic acid, HA, was dissolved in sufficient water to make 50mL of solution and was titrated with a .135 M NaOH solution. After the addition of 10.6mL of base, a pH of 5.65 was recorded. The equivalence point was
The reactants have five molecules that contain two hydrogen and four molecules that contains one oxygen and one nitrogen. In the products there are two molecules that contain two nitrogen, four molecules that contain one oxygen and two hydrogen, and one
A sample of ethanol, C2H5OH, weighing 2.84 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25.00°C to 33.73°C. If the heat capacity of the calorimeter and contents was 9.63 kJ/°C, what is the value
Current is applied to an aqueous solution of calcium sulfide. Multiple choice help please??! What is produced at the cathode? A) H2(g) B) S(s) C) O2(g) D) Ca(s) What is produced at the anode? A) O2(g) B) H2(g) C) Ca(s) D) S(s)
Calculate the level from which the electron fell, n2, for the hydrogen line you observed. wavelength (lambda) = 400 nm n1 = 2 RH = 2.18 x 10^-18 I keep having trouble with finding n2. Is the above given right to plug in for 1/(lambda) = RH (1/n1^2 - n2^2)
The formula of zinc trioxocarbonate (iv)
A scuba diver’s tank contains 0.29 kg of O2 compressed into a volume of 2.3L. A)calculate the gas pressure inside the tank at 9 Celsius. B) what volume would this oxygen occupy at 26 Celsius and 0.95atm? Answer is a)91atm B) 2.3 x 10^2 L Trying to find
a gas at 10atm pressure occupy a volume of 10L at 300k it is allowed to expand at the constant temperature of 300k under constant external pressure till the volume equilibrate at 100L calculate the work done
Calculate the volume of solution that has a vapour pressure of 31.27 mbar and contains 84.3g of sucrose, at a temperature of 25.0C. The vapour pressure of pure water at 25.0C is 31.7mbar, the density of water is 1.00g/mL, and assume no change in volume
(Iron ore is impure Fe_2O_3. When Fe_2O_3 is heated with an excess of carbon (coke), metallic iron and carbon monoxide gas are produced. From a sample of ore weighing 950kg , 533kg of pure iron is obtained). What is the mass percent by mass, in the ore
1000cm3(cude) of air at 20C and 101.35kpa is heated at constant pressure until its volume doubles. (A) use the ideal gas equation to calculate the final temprature of the gas? (B) calculate the work done by the gas as it expands.
Kc for the reaction of hydrogen and iodine to produce hydrogen iodide, H2(g)+I2(g)f 2HI(g) is 54.3 at 430C. What will the concentrations be at equilibrium if we start with 0.240M concentrations of both H2 and I2?
(a) How many excess electrons must be distributed uniformly within the volume of an isolated plastic sphere 30.0 cm in diameter to produce an electric field of 1150 N/C just outside the surface of the sphere? (b) what is the electric field at a point 10.0
A 26.0 kg block is connected to an empty 1.00 kg bucket by a cord running over a frictionless pulley. The coefficient of static friction between the table and the block is 0.490 and the coefficient of kinetic friction between the table and the block is
To what pH should you adjust a standard hydrogen electrode to get an electrode potential of -0.124V V ? (Assume that the partial pressure of hydrogen gas remains at 1 atm.)
Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCl. Calculate the pH after the following volumes of titrant have been added: a. 61.0 mL b. 65.0 mL im having a hard time even starting this question so any help would be greatly appreciated.
At 22 °C an excess amount of a generic metal hydroxide M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 10.56. What is the Ksp of the compound at 22 °C? I have found my [OH-] concentration (3.63x10^-4) but I'm not sure I'm
How many formula units are in 1.31 mg of hydrogen peroxide (H2O2)? Answer in units of formula units. For 508 g of butadiene (C4H6) calculate the number of moles. Answer in units of mol. Calculate the number of molecules. Answer in units of molec. 016 1.0
Hydrogen and chlorine react to yield hydrogen chloride: H2+ Cl2 ( 2HCl. How many grams of HCl are formed from reaction of 3.56 g of H2 with 8.94 g of Cl2? Which reactant is limiting?
A 26.0 kg block is connected to an empty 1.00 kg bucket by a cord running over a frictionless pulley (Fig. 4-57). The coefficient of static friction between the table and the block is 0.490 and the coefficient of kinetic friction between the table and the
Describe a simple laboratory experiment to distinguish between calcium hydrogen carbonate and sodium hydrogen carbonate
1.43g sample of potassium hydrogen phthalate [khp] required 24.11 cm3 or naoh for its completer neutralization. calculate the molarity of the naoh used in the titrationmple of
Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from the energy state of n=4 if it requires an energy of at least 1.36 x10^-19 J to do this. Please help with formulas to use?
RATES OF CHANGE QUESTION A spherical balloon is being blown up so that its volume is increasing by 0.6 m^3 s^-1. Find the rate at which the radius is increasing when the radius is 0.1 m. So what I did was that I determined dV/dt =0.6 and dV/dr = 4/3 r^3
Calculate the final concentration for the standardization of KMnO4 given this information: 2MnO4- + 5C2O4^-2 + 16H+ -> 2Mn^2+ + 10CO2 + 8H2O [final redox equation] Volume of KMnO4 titrated with H2SO4 + Na2C2O4 = 293 mL Volume KMnO4 titrated with H2SO4
An isotonic solution contains 0.86% by mass per volume. Calculate the percent mass per volume for an isotonic solution of KCl at 30 degrees C. Assume a van't Hoff factor of 1.9.
A rectangular block of wood floats in water with two-third of its volume immersed. When placed in another liquid, it floats with half of its volume immersed. Calculate the relative density of the liquid. (5
The equilibrium between three substances, a, B and c is shown below. A(g) + B(g) C(g) Initially there were 0.1 mol of a and 0.2 mol of B in the reaction mixture. a and B reacted together to produce an equilibrium mixture containing 0.04 mol of c. The total
The concentration of Pb2+ in a sample of wastewater is to be determined by using gravimetric analysis. To a 100.0-mL sample of the wastewater is added an excess of sodium carbonate, forming the insoluble lead (II) carbonate (267.2092 g/mol) according to
What is the y-coordinate of point b if the slope of line ab is 5. B(3,y). A(2,4) I added 3+2=5 and added +4=9 is this right
Current is applied to a molten mixture of CuF, ZnCl2, and AlBr3. What is produced at the cathode? a)F2 b)Al c)Cu d)Zn e)Cl2 f)Br2 What is produced at the anode? Same options as above.
4NH3 + 5O2 --> 4NO + 6H2O 170g of ammonia (NH3) are allowed to react with 384g of O2. how many moles of NO is produced? and also how many grams of NO will be produced?
If the mean value of the weight of a particular brand of dog food is 20.6 lb and the standard deviation is 1.3, assume a normal distribution and calculate the amount of product produced that falls below the lower specification value of 19.7 lb.
the pressure of hydrogen gas in a constant volume cylinder is 4.25atm at 0 degrees celsius. what will the pressure be if the temp. is raised to 80 degress celsius? Also do we have to first convert celsius to kelvin?
How many atoms are in Zinc Chloride, ZnCl2?
The easiest fusion reaction to initiate is 1-1H + 1-1H------> 4-2He + 1-0 n The 1-1 indicates a small one above the other on the left side of the symbol of the element.So for 1-0n is a one above a zero on the left side of n (neutron). The number on the top
Convert the following into a balanced equation: Liquid disilicon hexachloride reacts with water to form solid silicon dioxide, hydrogen chloride gas, and hydrogen gas.
. Calculate the following: a. the modulus of elasticity, b. the tensile strength, c. the fraction of the load carried by the fiber, for the following composite material stressed under isostrain conditions. The composite consists of a continuous
What volume of 0.123 M NaOH(aq) must be added to 125 mL of 0.197 M H2SO3(aq) to reach the following points? (a) the first stoichiometric point (b) the second stoichiometric point
what is the concentration of a solution made by mixing 22.0 g of salt with 200 mL of water? assume that the volume of the water does not change when the salt is added
Calculate the number of coulombs of positive charge in 261 cm3 of (neutral) water. (Hint: A hydrogen atom contains one proton; an oxygen atom contains eight protons.)
what is the Mr of CO2? Use this to calculate the mass of co2 produced when 1kg of CaCO3 is heated.... (what are the answers?) MT!!!
calculate the minimum concentration of ag+ ion that must be added to (or built up in) a 0.140 m Na2CrO4 solution in order to initiate a precipitation of silver chromate. The ksp of ag2cro4 is 1.2 × 10^-12.
Suppose it takes 35 min for 2.4 g of sugar to completely react with another reagent we added to the flask. What would the reaction rate be? Calculate to the correct number of significant figures.
Calculate the number of grams of CO2 is produced from 58.0g of glucose? ______g. CO2
Water is added to 200 cm3 of a 2.0 M solution of CaCl2 to increase the volume of the solution to 400 cm3. What is the new concentration?
A storage tank at stp contains 18.5kg of nitrogen. What is the volume of the tank and what would the pressure be if you added another 15kg of nitrogen at the same temperature?
5.6g of iron metal Fe are heated strong and mixed with 8g of sulfur S to form 4.4g of iron(ll) sulfide FeS. a, identify the limiting and excess reactants. b, calculate the mass of FeS formed. C,calculet the percent yield of FeS.
Copper metal reacts with concentrated nitric acid according to the following balanced equation: 3Cu(s) + 8HNO3(aq) �¨ 3Cu(NO3)2(s) + 2NO(g) + 4H2O(l) Calculate the mass in grams of the excess reagent remaining after the complete reaction of 4.63 g of Cu
A buffer is prepared by mixing 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 M HF (Ka = 6.8x10^-4) Calculate the pH of this buffer after 5.0 mL of 0.05 M HCl is added.
A 20ml sample of .125M diprotic acid solution was titrated with .1019M KOH.the constants for the acid are k1=5.2*10 ^-5 and K2=3.4*10 ^-10. What added volume of base does each equivalence point occur? i got .0254L for the first one and .0508 for the
what volume of oxygen at 423.0K and a pressure of 127.4kPa will be produced by the decomposition of 129.7g barium peroxide to form barium oxide and oxygen gas? Thank you
To 1.0 L of a 0.38 M solution of HClO2 is added 0.18 mol of NaClO. Calculate the [HClO2] at equilibrium.
A balloon contains 10.0g of neon gas. With T kept constant, 10.0g of argon gas is added, and the volume of the balloon expands by less than 2 times. Why?
You have 75.0 mL of a 2.50 M solution of Na2CrO4 (aq). You also have 125 mL of a 2.15 M solution of AgNO3 (aq). Calculate the concentration of NO3 when the two solutions are added together.
Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCl. Calculate the pH after the following volumes of titrant have been added. (The Kb for NH3 is 1.8e-05.) (a) 0 mL . (b) 25.0 mL . (c) 59.0 mL . (d) 60.0 mL (e) 63.0 mL (f) 67.5 mL
In an experiment to find the percentage of calcium carbonate in sand from a beach, 1.86 g of sand reacted with an excess of dilute hydrochloric acid to give 0.55 g of carbon dioxide. CaCO3 (s) + 2HCL (aq) – CaCl2(aq) + CO2(g) + H2O (l) 1.Calculate the
A buffer solution is prepared by mixing 99.0 mL of 0.450 M HF and 55.0 mL of 1.15 M NaF. Determine the pH of the solution after the addition of 0.01 moles NaOH (assume there is no change in volume when the NaOH is added).
What mass of NaF must be added to 1.0 L of 0.0036 M Pb2+ to initiate precipitation of PbF2(s)? (Ksp of PbF2 is 3.3 × 10-8; assume no volume change on addition of NaF.) can you please explain
A 1.500-g sample of a mixture containing only Cu2O and CuO was treated with hydrogen to prduce 1.252 g pure copper metal. Calculate the percentage composition (by mass) of the mixture.
A 1.00 g sample of limestone is allowed to react with 100 cm^3 of 0.200 mol/dm^3 HCl. The excess acid required 24.8 cm^3 of 0.100 mol/dm^3 NaOH solution. Calculate the percentage of calcium carbonate in the limestone
Please help! What are the differences between zinc carbon and alkaline batteries?
In a zinc-copper cell, Zn | Zn+2(1M) || Cu+2(1M) | Cu, which electrode is negative? a. Cu(s) b. Zn(s) c. Zn+2(aq) d. Cu+2(aq) Its A or C. Not sure. Please help.
Calculate the pH for the hydrogen half-cell of the following voltaic cell if the observed cell voltage is 1.00 V. Mn|Mn2+(1.00 M)||H+(pH =?), H2(1.00 atm)|Pt
How would you distinguish between calcium hydrogen carbonate and sodium hydrogen carbonate without using any lab chemical
A rectangular tank of 5 m long,4 m wide and 5 m high is filled with water to a depth 3 m. If a robot of volume 20 cubic metre is added to the tank, how much will the water level rise?
Sodium chloride is added to water (at 25⁰C) until it is saturated. Calculate the Cl- concentration in such a solution. Useful data are provided below. ∆G⁰f (kJ/mole): NaCl (s) -384 Na+ (aq) -262 Cl- (aq) -131
Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the following endothermic reaction:
I have to calculate the concentration of I2 produced (# of moles of I2 produced / L) based on the stoichiometric ratio in the following equation. 2S2O3^2- + I2 -> 2I^- + S4O6^2- Chemistry(Urgent, please help) - DrBob222, Sunday, February 26, 2012 at 9:47pm
Calculate the pH when the following volumes of 10^(-1,1) M XOH are added into 1 L of a 10^(-2.5) M HA solution. XOH is a strong base and HA is a weak monoprotic acid (pKa=4.5)
two cylindrical tanks have the same height, but the radius of one tank equals the diameter of the other. if the volume of the larger is k% more than the volume of the smaller, k= ? a)50 b)100 c)200 d)300 e)400 small tank volume: pi*(r/2)^2*h big tank
calculate the theoretical yield (in grams) of the solid product, assuming that you use 1.0 g FeC2O4×2H2O and that oxygen is the excess reactant. FeC2O4×2H2O (s) + O2(g) ---> FeO(s) + H2O(g) + CO2(g) Its balanced equation is 2FeC2O4×2H2O (s) + O2(g)---->
Excess electrons are placed on a small lead sphere with mass 8grams so that its net charge is -3.20*10^9C. a) Find the number of excess electrons on the lead sphere b) How many electrons are there per lead atom
Endothermic reaction equilibrium: BiCl3(aq) + H2O(g) = BiOCl(s) +2HCL(aq) + 2 HCl at a point at which the sollution is colorless and a small minute amoount of BiOCl(s) is observed. for the folowing questions 1to 5: a. state which way the reaction shift in
An empty relative density bottle weighs 25g.it weighs 65g when filled with a liquid and 75g when with water.caculate the density of the liquid.
When a force of 50N is applied to the free end of an elastic cord, an extension of 4cm is produced. Calculate the work done on the cord.
combustion analysis of a hydrocarbon produced: 33.01 g CO2 and 13.51 g H2O Calculate the empirical formula of the Hydrocarbon. I got CH5 but that doesn't seem right? how do i do this problem?
10000 tonnes of iron reacted in a blast furnace Fe2O3 calculate the typical mass of iron produced each day
Iron has a density of 7.86 g/cm3 (1 cm3=1 mL). Calculate the volume (in dL) of a piece of iron having a mass of 3.97 kg . Note that the density is provided in different units of volume and mass than the desired units of volume (dL) and the given units of
The density of an aqueous solution containing 10% of ethanol (C2H5OH) by mass is 0.984 g/ml. A) Calculate the molality of this solution. B) Calculate its molarity. C) What volume of the solution would contain 0.125 mol of ethanol.
What is the maximum mass (in grams) of each of the following soluble salts that can be added to 120 mL of 0.050 M BaCl2 without causing a precipitate to form? (Assume that the addition of solid causes no change in volume.) (a) (NH4)2SO4 × 10 g (Enter your
1.) A convenient method of determining the volume of a container of irregular shape is to fill it with a liquid of known density and measure the mass. An empty Erlenmeyer flask marked "10 mL" weighs 26.3251 g. When filled with mercury, with density =
Calculate the number of grams of calcium chloride (CaCl2) needed to react with excess silver nitrate (AgNO3) to produce 6.60 g of silver chloride (AgCl). The equation for the reaction is given below: CaCl2 + 2AgNO3 → 2AgCl + Ca(NO3)2
if 465cm cube of so2 can diffuse through a porous partition in 30sec how long will (a) an equal volume (b) 630cm cube of hydrogen sulphide take to diffuse through the same partition
If 465 cm cube of sulphur(iv)oxide,can diffuse through porous partition in 30 seconds,how long will an equal volume , 620 cm cube of hydrogen sulphide take to diffuse through the same partition?(H=1, S=33, O=16)
Given the following dissolving process: Fe2(SO4)3 (s) = 2Fe3+ (aq) + 3SO42- (aq) How many grams of iron (III) ions are produced when 0.450 moles of sulfate ion are produced? options: 50.3 g 16.8 g 50.3 g 37.7 g 75.4 g
A 0.25g sample of a pretzel is burned. The heat it gives of is used to heat 50.g of water from 18 to 42 degrees C. what is the caloric value of the pretzel in kcal/g? Can someone walk me through step by step?
An industrial engineer has found that the standard household light bulbs produced by a certain manufacturer have a useful life that is normally distributed with a mean of 250 hours and a variance of 2500. (a) What is the probability that a randomly
A 1.00-mole sample of ammonia at 13.0 bar and 20°C in a cylinder fitted with a movable piston expands against a constant external pressure of 1.00 bar. At equilibrium, the pressure and volume of the gas are 1.00 bar and 22.0 L, respectively. a) calculate
1000 cm3 of air at 20 temperature and 101.35 kpa is heated at constant pressure until its volume doubles. a, use the ideal gas equation to calculate the final temperature of the gas. b, calculate work done by the gas as it expands.
pls help. A weak acid HA (pKa = 5.00) was titrated with 1.00 M KOH. The acid solution had a volume of 100.0 mL and a molarity of 0.100 M. Find the pH at the following volumes of base added and make a graph of pH versus Vb: Vb = 0, 1, 5, 9, 9.9, 10, 10.1,
A water chemist obtained a 250 ml sample from a nearby lake and fixed the oxygen on-site with alkaline solutions of MnSO4 and KI-NAN3. Returning to the laboratory, a 200 ml sample was analyzed by acidifying the sample with conc H2SO4 and then titrating

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Calculate the change in enthalpy produced by dissolving 14.3 g of NaOH in 65.0 g of water if the temperature increases 49.1°C and the specific heat of water is 4.18 J/g°C I believe you multiply 4.18, 65.0, and 49.1. Am I correct
When 11.0 g of calcium metal is reacted with water, 5.00 g of calcium hydroxide is produced. Using the following balanced equation, calculate the percent yield for the reaction? Ca(s) + 2 H2O(l) → Ca(OH)2(aq) + H2(g) 84.0% 12.3% 45.5% 24.6%
Calculate the total number of moles of gas produced from the decomposition of 10.0 g of guanidinium nitrate I know that the equation for the decomposition is CH6N4O3 (s) → 3 H2O (g) + 2 N2 (g) + C but I don't know where to go from here.
Calculate the number of GRAMS of carbon dioxide (CO2) produced when 100 grams of methane (CH4) are completely burned in oxygen (O2).
How much ml of H2So4 added to make 0.02M H2So4 solution to make volume 250ml?
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O3(g)+NO(g) --> O2(g)+NO2(g) The rate law for this reaction is: rate=k[O3][NO] Given that k = 2.87 × 106 M–1·s–1 at a certain temperature,
100.0 g of copper(II) carbonate (molar mass = 123.56 g/mol) was heated until it decomposed completely. The gas was collected and cooled to room temperature and normal pressure (25¨¬C and 1.00 atm). What volume of carbon dioxide was produced? The reaction
An organic compound A contain 62.0% by mass of carbon, 21.1% by mass of nitrogen, the reminder being hydrogen. Determine the percentage by mass of hydrogen and the empirical formula A.....Can any one help me on that?????
At what temp do hydrogen molecules, H2, have the same rms speed as nitrogen molecules, N2, at 455 C? At what temperature do hydrogen molecules have the same average kinetic energy?
Based on the following chemical equation, balance the equation an answer the following questions: Fe2(S04)3 + NaCl ( FeCl3 + Na2S04 Calculate the amount in grams of NaCl needed to produce 75 g of FeCl3. Calculate the amount of Fe2(S04)3 in grams produce
Calcium carbonate CaCO3 reacts with stomach acid (HCl, hydrochloric acid) according to the following equation: CaCO3(s)+2HCl(aq)->CaCl2(aq)+H2O(l)+CO2(g) Tums, an antacid, contains CaCO3. If Tums is added to 35.0 mL of 0.300 M HCl,how many grams of CO2 gas
The reaction of calcium bicarbonate, Ca(HCO3)2 with hydrochloric acid, HCl, produces a solution of CaCl2, gaseous carbon dioxide, CO2, and water, H2O. Write a balanced chemical equation for this reaction and determine the volume of CO2, in mL, that forms
When 2 moles of ammonia (NH3) decomposes into nitrogen gas (N2) and hydrogen gas (H2), how many moles of NITROGEN gas are produced? 1 mole 2 moles 3 moles 4 moles I was thinking 2 moles?
6.70 A sample of benzene, C6H6, weighing 3.51g was burned in an excess of oxygen in bomb calorimeter. The temperature of the calorimeter rose from 25.00C to 37.18C. If the heat capacity of the calorimeter and contents was 12.05kJ/C, what is the value of q
Using the correct number of significant figures, calculate the perimeter and volume of a small, rectangular mirror that is 4.040 in long, 1.707 in wide, and 0.078 in thick. Make sure to calculate the the perimeter of the front of the mirror, and not the
A student constructs a galvanic cell that has a strip of iron metal immersed in a solution of 0.1M Fe(NO3)2 as one half-cell and a strip of zinc metal immersed in a solution of 0.1M Zn(NO3)2 as the other half-cell. The measured cell potential is less than
A saturated solution is prepared by adding excess PbI2(s) to distilled water to form 1.0L of solution at 25oC. The concentration of Pb+2 in the saturated solution is found to be 1.3*10-3 M. Calculate the Ksp for PbI2(s) in water at 25 °C R/
The fizz produced when an Alka-Seltzer® tablet is dissolved in water is due to the reaction between sodium bicarbonate (NaHCO3) and citric acid (H3C6H5O7): In a certain experiment 1.45g of sodium bicarbonate and 1.45g of citric acid are allowed to react.
Sodium metal reacts violently with water to form NaOH and release hydrogen gas. Suppose that 3.00 g of Na reacts completely with 3.00 L of water and the final volume of the system is 3 L. What is the molarity M of the NaOH Solution formed by the reaction?
.Balance the chemical equation given: zinc oxide+ sulphuric (vi) acid
Which one of the following is an alkaline earth element? a) carbon b)sodium c)zinc d)iron
What is the net ionic equation of the rection between zinc and copper 2 sulfate?
what is the experimental errors in determining the formula unit of zinc chloride?
Can you please tell me if this is a balanced equation for Zinc and acetic acid... Zn(s) + 2CH3COOH(aq)-->Zn(aq)(CH3COO)2 + H2(g) I would appreciate any help
Equation For The Reaction Between Zinc Metal And Dilute Tetraoxosulphate (vi) Acid
what mass of zinc will be required to react completely with 100cm3 of a 1.0M hcl.
a buffer composed of 0.50mol acetic acid and 0.50mol sodium acetate is diluted to a volume of 1.0L. The pH of the buffer is 4.74. How many moles of NaOH must be added to the buffer solution to increase its pH to 5.74?
Consider the combustion of propane: C3H8(g)+5O2(g) yields 3CO2(g) + 4H2O(l) delta H= -2221 kJ Assume that all of the heat comes from the combustion of propane. Calculate delta H in which 5.00g of propane is burned in excess oxygen at constant pressure.
Consider the combustion of propane: C3H8(g)+5O2(g) yields 3CO2(g) + 4H2O(l) delta H= -2221 kJ Assume that all of the heat comes from the combustion of propane. Calculate delta H in which 5.00g of propane is burned in excess oxygen at constant pressure.
A 5.00 L solution has [HC7H5O2] = 0.100 M and [Ca(C7H5O2)2] = 0.200 M . What is the pH of the solution after 10.0 mL OF 5.00 M NaOH is added? Assume the volume of the solution does not change .Ka for HC7H5O2 = 6.3x10^-5.
How much alfalfa should be added to 60L of ostrich pellets to create a mix that is 32% alfalfa by volume? I have no idea how to start this question. If I let x be the alfalfa and x+60 = 32 be the mix
Balance the chemical equation for the important industrial process: C2H4 + O2 + HCl → C2H4Cl2 + H2O. Given 610.0 kg of hydrochloric acid, calculate how many kg of C2H4Cl2 can be produced.
a cuboid with length 13cm width 4cm and height h State in terms of h the shaded face of the cuboid. write an expression in terms of h for the volume of the cuboid. if the volume of the cuboid is 286cm cube calculate the height h of the cuboid.
Under the same condition temperature and pressure hydrogen diffuses 8 times as fast as gas y calculate the rmm of gas y the rmm of h=2
Very small crystals composed of 1000 to 100,000 atoms, called quantum dots, are being investigated for use in electronic devices. (a) Calculate the mass in grams of a quantum dot consisting of 1.400 104 atoms of silicon. (b) Assuming that the silicon in
In an excess of NH3(aq), Cu2+ ion forms a deep blue complex ion, Cu(NH3)42+, which has a formation constant Kf = 5.6 1011. Calculate the Cu2+ concentration in a solution prepared by adding 4.8 10-3 mol of CuSO4 to 0.500 L of 0.32 M NH3.
Sulfur dioxide reacts with oxygen to form sulfur trioxide according to the equation 2SO2(g) + O2(g) 2SO3(g) Samples of sulfur dioxide, oxygen, and sulfur trioxide were added to a flask of volume 1.40 dm^3 and allowed to reach equilibrium at a given
I am really having trouble answering this question, can someone help? A binary compound between an unknown element E and hydrogen contains 91.27% E and 8.73% H by mass. If the formula of the compound is E3H8, calculate the atomic mass of E.
Solubility of Calcium Hydroxide At some temperature, the solubility of Ca(OH)2 is 0.0880 g/100mL. Calculate the concentrations of the Ca2+ and OH− ions in a saturated solution of Ca(OH)2 and use these to calculate a value for Ksp of Ca(OH)2. [Ca^2+]=
Calculate the volume of NaOH 0.5 mol/L necessary to neutralize 300 mL of HCl 0.2 M. na= how do I calculate this? Ma= 0.2 M Va= 0.300 L nb= 0.5 mol Mb= 0.5 M Vb= ?
Calcium nitrate will react with ammonium chloride at slightly elevated temperatures, as represented in the equation Ca(NO3)2(s) + 2NH4Cl(s) ---> 2N2O(g) + CaCl2(s) + 4H2O(g) What is the maximum volume of N2O at STP that could be produced using a 6.80-mol
What do positive hydrogen ions produce when they react with water in solution? A).hydroxide ions B).hydronium ions C).a salt D).negative hydrogen ions I believe the answer is A). Is this correct?
In a water molecule, two hydrogen atoms bind to one oxygen atom. How many lone pairs of electrons will be shown around each hydrogen atom in the Lewis structure of water?
Consider the following chemical reaction: C (s)+ H2O(g) --> CO(g)+ H2(g) How many liters of hydrogen gas are formed from the complete reaction of 1.20 mol of C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and temperature of 310 K.
At a high temperature, the equilibrium constant for the decomposition of hydrogen iodide is 65.0. If the initial concentration of HI is 1.60 M, what is the concentration of hydrogen at equilibrium? 2Hl(g) H2(g) + I2(g) A. 1.42 M B. 0.753 M C. 0.240 M D.
Calculate the masses of Cr2O3, N2, H20 produced from 10.8 g (NH4)2Cr2O7 [ the 2 belongs to the nh4] in an ammonium dichromate volcano reaction. I need to know what the balance equation is, and im having a little trouble with it. Pleasee help!
Heat is given off when hydrogen burns in air according to the equation: 2H2 + O2 ---> 2H2) What is responsible for the heat? I know the answer is froming hydrogen-oxygen bonds gives off energy, but why?
In the explosion of a hydrogen-filled balloon, 0.30g of hydrogen reacted with 2.4g of oxygen to form how many grams of water vapor? (Water vapor is the only product.)
Formic acid ,HCOOH, is a monoprotic acid. circle the acidic hydrogen. Write the formula of the conjugate base after the acidic hydrogen is lost.
Hydrogen atoms are excited to the stationary state designated by the principal quantum number, n= 4. What will be the number of lines(frequencies) emitted by the hydrogen atoms?
Prior to their phaseout in the 1980s, chemicals containing lead were commonly added to gasoline as anti-knocking agents. A 3.279 g sample of one such additive containing only lead, carbon, and hydrogen was burned in an oxygen rich environment. The products
A buffer was prepared by mixing 1.00 mol of ammonia 𝑁𝐻3 𝐾𝑎 = 5.8 × 10−10 and 1.00 mol of ammonium chloride 𝑁𝐻4𝐶𝑙 to form an aqueous solution with a total volume of 1.00 liter. To 500 mL of this solution was added 30.0 mL of 1.00
How would one calculate the equilibrium pressure of Sodium bicarbonate and citric acid in water (think Alka Seltzer), reacting in a closed volume. The pressure builds up to a point, where the reaction slows due to pressure build up. How do I calculate the
Finish the equation: Solutions of zinc sulfate and sodium phosphate are mixed
Sodium thiosulfate, Na2S2O3, is an important reagent for titrations. Its solutions can be standardized by titrating the iodine released when a weighed amount of potassium hydrogen iodate, KH(IO3)2 (389.912 g/mol), is allowed to react with excess potassium
Ten identical lengths of wire are laid closely side by side. Their combined width is measured and found to be 14.2 mm. Calculate: a)the radius of a single wire b)the volume in mm cubed of a single wire if its length is 10.0 cm. (Volume of a cylinder =
Freon-12 is formed as follows: 3 CCl4 + 2 SbF3 -> 3 CCl2F2 + 2 SbCl3 150 g tetra chloromethane is combined with 100 g antimony (III) fluoride to give Freon-12 (CCl2F2). Identify the limiting and excess reagents, and calculate how many grams of Freon-12 can
Calculate the volume of Ba(OH)2 0.20 M necessary to neutralize 300.0 mL of H3PO4 0.30 M. (4 marks)
Calculate The volume occupied at s.t.p by 0.24g of ozone ( o=16, G.M.V=22.4dm3
Given the molar concentration of hydroxide ion, calculate the concentration of hydrogen ion. [OH-]=0.0010 Can someone please help me with this process. Thanks
1. 25mL of 0.1M HCl is titrated with 0.1M NaOH. What is the pH when 30mL of NaOH have been added? 2. 25mL of 0.1M HCl is titrated with 0.1M NaOH. What is the pH after 15mL of NaOH have been added? I don't know how to make calculation I assumed that for
During the electrolysis of molten aluminum chloride in an electrolytic cell, 5.40 g of aluminum is produced at the cathode. Predict the mass of chlorine produced at the anode.
1. If a student fails to remove a large air bubble in the buret before beginning the titration, what will be the effect on the volume of titrant required to reach the titration endpoint? A. The student will record a volume that is SMALLER than it should be
The pH of a chemical solution is given by the formula pH = -log10 [H+] where [H+] is the concentration of hydrogen ions in moles per liter. Values of pH range from 0 (acidic) to 14 (alkaline). (a) what is the pH of the solution for which [H+] is 0.1? (b)
Aluminum oxide is formed by reaction of excess oxygen with aluminum. 4 Al(s) + 3 O2(g) -> 2 Al2O3(s) Calculate the mass of aluminum required to form 18.2 kg of aluminum oxide if the reaction has a percent yield of 83.4%.
What are the differences between proteins produced in free ribosomes versus proteins produced in the rough endoplasmic reticulum?
In transporting a patient on a wheelchair up an inclined ramp at an angle of 20° with the horizontal ground, an attendant exerts a force of 1400N, resulting in a velocity of 2.5 m/s. Calculate the power produced by the attendant.
Calculate the mass of water in grams that could be produced from the reaction of 10.00mL 0.4122M hydrochloric acid and 35.00mL 0.1738M sodium hydroxide solution. Identify the limiting reactant.
Consider the following cell: Pt|H2(g, 0.460 atm)|H (aq, ? M)||Ag (aq, 1.00 M)|Ag(s) If the measured cell potential is 1.00 V at 25 °C and the standard reduction potential of the Ag /Ag half-reaction couple is 0.80 V, calculate the hydrogen ion
Help please, What is the minimum mass of NH4HS that must be added to the 5.00-L flask when charged with the 0.350g of pure H2s(g), at 25 ∘C to achieve equilibrium? Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the
Calculate the concentration of the cobalt(II) chloride hexahydrate solution titrated in the fine titration experiment. Show your calculations and provide answer with the appropriate number of significant figures. concentration of AgNO3 solution (mol/L)
N2(g)+3H2(g) -> 2NH3(g)+ 22000 cal Consider the reaction is at equilibrium. Explain how the equilibrium is shifted when a. more N is added b. more H is added c. ammonia is removed
Air consits of 21% oxygen, 78% nitrogen and 1% argon by volume. Calculate the partial pressures in Pa if total pressure is 1 atm. My teacher just converted 1atm in pa and then did 21% of that for oxygen etc etc. Can you explain why she did this, is volume
Carbon dioxide is usually formed when gasoline is burned. If 30.0 L of Co2 is produced at a temperature of 1.00 X 103 C and allowed to reach room temperature (25.0 C) without any pressure change, what is the new volume of the carbon dioxide?
Household hydrogen peroxide is an aqueous solution containing 3.0% hydrogen peroxide by mass. What is the molarity of this solution? (Assume a density of 1.01g/ml .)
The Norfolk Bank has $18,000 in excess reservces and the reserve ratio is 20 percent. Which level of checkable deposits and reserves might this bank hold? a. $160,000 in checkable-deposit liabilities and $47,000 in reserves. b. $140,00 in checkable-deposit
How many grams of NH4Cl must be added to 0.560 L of 1.90 M NH3 solution to yield a buffer solution with a pH of 8.50? Assume no volume change. Kb for NH3 = 1.8 10-5. i am confused as how to find the grams?
When .03 mol Na is added to 100g of water, the temp. of the resulting solution rises from 25C to 37.9C. If the specific heat of the solution is 4.18 J/(g C), calculate delta H for the reaction, 2Na(s) + 2H2O(l) --> 2NaOH(aq) + H2(g)
One mole of an ideal gas initially at a temperature of Ti = 7.4°C undergoes an expansion at a constant pressure of 1.00 atm to eight times its original volume. (a) Calculate the new temperature Tf of the gas.______J (b) Calculate the work done on the gas
A 0.552 g sample of ascorbic acid(Vitamin C) was dissolved in water to a total volume of 20.0 ml and titrated with 0.1103 M KOH. The equivalence point occurred at 28.42 ml. The pH of the solution at 10.0 ml of added base was 3.72. From this data, determine
How long (in minutes) must a 5.40 A current be passed through an aqueous solution of zinc nitrate to deposit 87.5 g Zn?
How long (in minutes) must a 5.40 A current be passed through an aqueous solution of zinc nitrate to deposit 87.5 g Zn?
What is the least reactive with aqueous solutions of metal ions? A. tin B. zinc C. gold D. calcium
If 18.0g of CO2 is produced in the reaction of C2H2 with O2 to form CO2 and H2O how many grams of H2Oare produced
Calculate surface area and the volume of a box that is 3m by 2m by 7.5m Show me how to get the answer please.
Calculate the volume at STP of these compounds 1,5 mol oxygen gas
calculate volume of cone with height 6cm and radius 10cm
Calculate the density of an object having a mass of 17g and a volume of 3 cm cubed. Thanks
Calculate the volume of conc .Hcl required for preparing 250ml 0.1M?
calculate the volume of a rectangular prism with a length of 5.6 , a width of 2.1 , and a height of 6.6 .
The volume of a sphere is increased by 6% calculate the corresponding percentage increase in the area.
Calculate the volume of 0.128 M HCl solution required to neutralize 2.32 g of Al(OH)3(s)
I wanted to calculate the normality of the acid and base solutions for a lab. But I'm extremely confused. I know normality is number of equivalents divided by volume in liters. But are we suppose to be given the number of equivalents of HCl and NaOH? Or
Iron has density 7.87 g/cm3. If 52.3 g of iron is added to 74.5 mL of water in a graduated cylinder, to what volume reading will the water level in the cylinder rise? mL
A solution contains 25 mmol of H3PO4 and 10. mmol of NaH2PO4. What volume of 2.0 M NaOH must be added to reach the second equivalence point of the titration of the H3PO4 with NaOH?
Liquid carbon disulﬁde reacts with 415 mL of oxygen to produce the gases carbon dioxide and sulfur dioxide. What volume of carbon dioxide is produced? Answer in units of L
A is a solution of HCL containing 7.30g/dm3.B is a solution ofX2CO3 containing 10.6g/dm3.assume that average volume of acid is 2.81cm3 and the volume of base is 25.00cm3.from your result and information .calculate (I)concentration of A in
Chemicals Reaction Online Practice Which option is an example of a chemical change? - baking a cake A scientist is using a lithium ion battery to power her laptop. Which statement about the battery is correct? -A new substance is formed as the battery is
How will the following system at equilibrium shift in each of the following cases? 2 SO3(g) 2 SO2(g) + O2(g) H° = 197 kJ (a) SO2(g) is added (b) the pressure is decreased by increasing the volume of the container (c) the pressure is increased by adding
Calculate the pH of a solution prepared by dissolving 10.0 g of tris(hydroxymethyl)aminomethane ("tris base") plus 10.0 g of tris hydrochloride in 0.250 L of water. (a) What will be the pH if 10.5 mL of 0.500 M NaOH is added?