How much volume of oxygen will be required for complete combustion of $40 m L$ of acetylene $(C_{2} H_{2})$ and how much volume of carbon dioxide will be formed? All volumes are measured at NTP

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Solution

$C_{2} H_{2} + \frac{5}{2} O_{2} ⟶ 2 C O_{2} + H_{2} O$
$1$ mole of $C_{2} H_{2}$ reacts with $\frac{5}{2}$ moles $O_{2}$ .
$∴$ Volume ratio of $C_{2} H_{2} : O_{2} =$ Mole ratio $= 1 : \frac{5}{2}$
$∴$ Value of $O_{2}$ required $= \frac{5}{2} \times 40 = 100 m l$ $O_{2}$ .
Volume ratio of $C_{2} H_{2} = C O_{2} =$ Mole ratio of $C_{2} H_{2} : C O_{2} = 1 : 2$
$∴$ Volume of $C O_{2}$ formed $= 2 \times 40 = 80 m l$ $C O_{2}$ .

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