Question

When methane ( CH4 ) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction isCH4(g)+O2(g)→CO2(g)+H2O(g) This type of reaction is referred to as a complete combustion reaction.What mass of carbon dioxide is produced from the complete combustion of 5.90×10−3 g of methane?Express your answer with the appropriate units.

Answer 1

1) Balance the chemical equation.

`CH_4+2O_2\rightarrow CO_2+2H_2O`

2) Convert the mass of CH4 to moles of CH4.

The molar mass of CH4 is 16.0425 g/mol.

`mol\text{ }CH_4=5.90*10^(-3)\text{ }g\text{ }CH_4*\frac{1\text{ }mol\text{ }CH_4}{16.0425\text{ }g\text{ }CH_4}=0.0003678\text{ }mol\text{ }CH_4`

3) Moles of CO2 produced from CH4.

The molar ratio between CH4 and CO2 is 1 mol CH4: 1 mol CO2.

`mol\text{ }CO_2=0.0003678\text{ }mol\text{ }CH_4*\frac{1\text{ }mol\text{ }CO_2}{1\text{ }mol\text{ }CH_4}=0.0003678\text{ }mol\text{ }CO_2`

4) Convert moles of CO2 to mass of CO2.

The molar mass of CO2 is 44.0095 g/mol.

`g\text{ }CO_2=0.0003678\text{ }mol\text{ }CO_2*\frac{44.0095\text{ }g\text{ }CO_2}{1\text{ }mol\text{ }CO_2}=0.0161855\text{ }g\text{ }CO_2`

The mass of CO2 produced from 5.90*10^-3 g CH4 is 0.0162 g CO2.

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