Question:
The formula of a gaseous hydrocarbon which requires 6 times of its own volume of $\mathrm{O}_{2}$ for complete oxidation and produces 4 times its own volume of $\mathrm{CO}_{2}$ is $\mathrm{C}_{\mathrm{x}} \mathrm{H}_{\mathrm{y}}$. The value of $\mathrm{y}$ is
Solution:
Combustion $\mathrm{rx}^{\mathrm{n}}$ :
$\mathrm{C}_{\mathrm{x}} \mathrm{H}_{\mathrm{y}(\mathrm{g})}+\left(\mathrm{x}+\frac{\mathrm{y}}{4}\right) \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{x} \mathrm{CO}_{2}(\mathrm{~g})+\frac{\mathrm{y}}{2} \mathrm{H}_{2} \mathrm{O}(\ell)$
Sinc : (I) $\mathrm{Vo}_{2}=6 \times \mathrm{V}_{\mathrm{C}_{\mathrm{x}} \mathrm{H}_{\mathrm{y}}}$
$\Rightarrow \mathrm{V}\left(\mathrm{x}+\frac{\mathrm{y}}{4}\right)=6 \mathrm{~V}$
