${CH}_{4} (g) + 2 O_{2} (g) ⟶ {CO}_{2} (g) + 2 H_{2} O (g)$
How many moles of methane are required to produce 22 g ${CO}_{2} (g)$ after combustion?

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I mol

0.5 mol

O.25 mol

1.25 mol

answer is B.

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Detailed Solution

According to the chemical equation

${CH}_{4} (g) + 2 O_{2} (g) ⟶ {CO}_{2} (g) + 2 H_{2} O (g)$

$44 {gCO}_{2} (g) is obtained from 16 {gCH}_{4} (g)$

$[∵ 1 mole {CO}_{2} (g) is obtained from 1 mole of {CH}_{4} (g)]$

$Mole of {CO}_{2} (g) = \frac{22 {gCO}_{2} (g)}{44 {gCO}_{2} (g)}$

= $0.5 mole {CO}_{2} (g)$

$Hence, 0.5 mole {CO}_{2} (g) would be obtained from 0.5 mole$ ${CH}_{4} (g) or 0.5 mole of {CH}_{4} (g) would be required to$ $produce 22 {gCO}_{2} (g) .$

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