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  4. Equal masses of SO2 CH4 and O2 are mixed in an empty container at 298 K, when total pressure is 2.1 atm. The partial pressure of CH4 in the mixture is

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Q. Equal masses of $SO_{2} CH_{4}$ and $O_{2}$ are mixed in an empty container at $298\, K$, when total pressure is 2.1 atm. The partial pressure of $CH_{4}$ in the mixture is

States of Matter

Solution:

Let $w\, g$ of each $SO_{2} CH_{4}$ and $O_{2}$ are mixed.
$\therefore $ Mole fraction,
$X_{CH_4} = \frac{n_{CH_4}}{n_{SO_2} +n_{CH_4} +n_{O_2}}$
$- \frac{\frac{w}{16}}{\frac{w}{64} +\frac{w}{16} +\frac{w}{32}} = \frac{4}{7}$
(Molecular weight of $SO_{2} = 64 u, CH_{4} = 16 u, O_{2} = 32 u$) Partial pressure of $CH_{4}$
$P_{CH_4}$ = Mole fraction $\times$ Total pressure$\frac{4}{7} \times 2.1 = 1.2\, atm$