What mass of carbon dioxide is produced from the complete combustion of 2.70 10 3 g methane?

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Michael S.

Chemistry 101

11 months, 2 weeks ago

We don’t have your requested question, but here is a suggested video that might help.

1. Calculate the percent by mass of Carbon in CO2? Report your answer with 3 significant figures. 2. What mass of Carbon Dioxide (CO2) is produced from the complete combustion of 32.5 g of Methane (CH4)?

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We don’t have your requested question, but here is a suggested video that might help.

What mass of CO2 is produced from the combustion of 65.3 grams of CH4? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) Please show all steps and explanation! thanks

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We first need to write down the balanced equation for this reaction, that is

#CH_4(g)+2O_2(g)->CO_2(g)+2H_2O(g)#

As we can see here, the mole ratio between methane #(CH_4)# and carbon dioxide #(CO_2)# is #1:1#, i.e. one mole of methane will produce one mole of carbon dioxide in return.

In here, we burn #2.6*10^-3 \ "g"# of methane. So, we need to convert that amount into moles.

Methane has a molar mass of #16 \ "g/mol"#. So, in here, we have

#(2.6*10^-3cancel"g")/(16cancel"g""/mol")=0.0001625~~1.63*10^-4 \ "mol of" \ CH_4#

Since the mole ratio between the two compounds is #1:1#, then we will also produce #1.63*10^-4# moles of carbon dioxide.

Carbon dioxide has a molar mass of #44 \ "g/mol"#.

So, the mass of carbon dioxide produced is

#1.63*10^-4cancel"mol"*44 \ "g/"cancel"mol"=0.007172 \ "g"#

Now, we can convert into scientific notation, which will be

#7.17*10^-3 \ "g"#

Since this answer asks us to give the answer in appropriate units, I suggest you use milligrams as the answer, as #1 \ "g"=1*10^3 \ "mg"#.

#<=>7.17*10^-3 \ "g" = 7.17 \ "mg"#