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Dalton's Law of Partial Pressures

Gaseous mixtu...

Question

Gaseous mixture of contains $56 g$ of $N_{2},$ $44 g$ of ${C O}_{2}$ and $16 g$ of ${C H}_{4} .$ The total pressure of mixture is $720 a t m$ of $H g$ The partial pressure of ${C H}_{4}$ is:

A

75 a t m

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B

160 a t m

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C

180 a t m

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D

215 a t m

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Solution

The correct option is C $75 a t m$
According to Dalton's Law of Partial pressure,
Partial pressure of $C H_{4} = (X_{C H_{4}}) \cdot P_{t o t a l}$
$X_{C H_{4}} = \frac{n o . o f m o l e s o f C H_{4}}{T o t a l n o . o f m o l e s} = \frac{\frac{16}{16}}{\frac{16}{16} + \frac{44}{44} + \frac{56}{14}} = \frac{1}{6}$
$⟹ P_{C H_{4}} = (\frac{1}{6}) (720)$ $a t m$
$⟹ P_{C H_{4}} = 120$ $a t m$

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