What volume of air (containing 20% $O_{2}$ by volume) will be required to burn completely $10 c m^{3}$ each of methane and acetylene.
$C H_{4} + 2 O_{2} ⟶ C O_{2} + 2 H_{2} O$
$2 C_{2} H_{2} + 5 O_{2} ⟶ 4 C O_{2} + 2 H_{2} O$

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Solution

$C H_{4} + 2 O_{2} ⟶ C O_{2} + 2 H_{2} O$
According to the reaction, 1 volume of $C H_{4}$ needs two volumes of oxygen is required. So, 10 cm $^{3}$ of $C H_{4}$ needs 20 cm $^{3}$ of oxygen. As air contains 20% oxygen, so 100 cm $^{3}$ of air is needed.
$2 C_{2} H_{2} + 5 O_{2} ⟶ 4 C O_{2} + 2 H_{2} O$
1 volume of $C_{2} H_{2}$ needs 2.5 volume of oxygen. So, 10 cm $^{3}$ of $C_{2} H_{2}$ needs 25 cm $^{3}$ of oxygen. As air contains 20% oxygen, so 125 cm $^{3}$ of air is required containing 25 cm $^{3}$ of oxygen.

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What volume of air (containing 20% O2 by volume) will be required to burn completely 10cm3 each of methane and acetylene.CH4+2O2⟶CO2+2H2O2C2H2+5O2⟶4CO2+2H2O

What volume of air (containing 20% $O_{2}$ by volume) will be required to burn completely $10 c m^{3}$ each of methane and acetylene.
$C H_{4} + 2 O_{2} ⟶ C O_{2} + 2 H_{2} O$
$2 C_{2} H_{2} + 5 O_{2} ⟶ 4 C O_{2} + 2 H_{2} O$