When burnt in air, $14.0 \mathrm{~g}$ mixture of carbon and sulphur gives a mixture of $\mathrm{CO}_{2}$ and…
When burnt in air, $14.0 \mathrm{~g}$ mixture of carbon and sulphur gives a mixture of $\mathrm{CO}_{2}$ and $\mathrm{SO}_{2}$ in the volume ratio of $2: 1$, volume being measured at the same conditions of temperature and pressure moles of carbon in the mixture is
$0.75$
$0.5$
$0.40$
$0.25$
Solution
Let weight of $\mathrm{C}$ be $\mathrm{xg}$, then $\mathrm{S}$ will be $(14-\mathrm{x}) \mathrm{g}$
$\frac{x / 12}{(14-x) / 32}=\frac{2}{1}$
$\therefore \quad \mathrm{x}=6 \mathrm{~g} ;$ Moles of $\mathrm{C}=\frac{6}{12}=0.5$