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Standard XII

Chemistry

Henry's Law

The air is a ...

Question

The air is a mixture of a number of gases. The major components are oxygen and nitrogen with approximate proportion of $20$ % to $79$ % by volume at $298 K$ . The water is in equilibrium with air at a pressure of $10 a t m$ . At $298 K$ , if the Henry's law constants for oxygen and nitrogen at $298 K$ are $3.30 \times 107 m m$ and $6.51 \times 107 m m$ respectively, calculate the composition of these gases in water.

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Solution

The vapour pressure of air over water is $10$ atm.

The partial pressure of nitrogen $= P_{N_{2}} = \frac{79 \times 10}{100} = 7.9 a t m = 7.9 \times 760 m m H g = 6004$ mm Hg

The partial pressure of oxygen $P_{O_{2}} = \frac{20 \times 10}{100} = 2.0 a t m = 2.0 \times 760 m m H g = 1520$ mm Hg

According to Henry's law,
$P_{N_{2}} = K_{H} (N_{2}) \times X_{N_{2}}$

$X_{N_{2}} = \frac{P_{N_{2}}}{K_{H} (N_{2})} = \frac{6004}{6.51 \times 10^{7}} = 9.22 \times 10^{- 5}$

$X_{O_{2}} = \frac{P_{O_{2}}}{K_{H} O_{2}} = \frac{1520}{3.30 \times 10^{7}} = 4.6 \times 10^{- 5}$

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