How many moles of methane are required to produced 22 g $C O_{2} (g)$ after combustion?

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Solution

$C H_{4} + O_{2} ⟶ C O_{2} + 2 H_{2} O$
Gram molecular mass of CO2 = 12 +2(16) = 44g/mol
From the reaction it is clear that 1 mole of methane on complete combustion produces 44g (1 mole) of carbon dioxide.
Therefore moles of $C H_{4}$ required to produce 22g of $C O_{2}$ are:
$= \frac{1}{44} \times 22 = 0.5 m o l$

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