Ethane C2H6 burns in oxygen to produce carbon dioxide and water as shown in the equation given below:
2C2H6 + 7O2 ⟶ 4CO2 + 6H2O
Calculate the composition of the resulting gaseous mixture at room temperature when 60 c.c. of ethane burns in 250 c.c. of oxygen.
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$$\begin{matrix} 2\text{C}_2\text{H}_6 & + & 7\text{O}_2 & \longrightarrow & 4\text{CO}_2 & + & 6\text{H}_2\text{O} \\ 2 \text{ vol.} & : & 7 \text{ vol.} & \longrightarrow & 4 \text{ vol.} & \\ \end{matrix}$$
[By Gay Lussac's law]
2 Vol. of C2H6 requires 7 Vol. of oxygen
∴ 60 cc C2H6 will require $\frac{7}{2}$ x 60
= 210 cc of Oxygen
Hence, unused oxygen = 250 - 210 = 40 cc
Similarly,
2 Vol. of C2H6 produces 4 Vol. of carbon dioxide
∴ 60 cc C2H6 produces $\frac{4}{2}$ x 60
= 120 cc of Carbon dioxide
Hence, carbon dioxide produced = 120 cc.
The gaseous mixture at room temperature (assuming water condenses) contains 120 cc CO2 and 40 cc O2.