The air is a mixture of a number of gases. The major components are oxygen and nitrogen with approximate proportion of `20%` is to `79%` by volume at 298 K. The water is in equilibrium with air at a pressure of 10 atm. At 298 K, if the Henry's law constants for oxygen and nitrogen are `3.30xx10^(7)` mm and `6.51xx10^(7)` mm respectively, calculate the composition of these gases in water.

Explanation

To solve the problem, we will use Henry's Law, which states that the amount of gas that dissolves in a liquid at a given temperature is directly proportional to the partial pressure of the gas above the liquid. The formula for Henry's Law is given by:

\[ C = k_H \cdot P \]

Where:
- \( C \) is the concentration of the gas in the liquid (in mm),
- \( k_H \) is the Henry's law constant for the gas (in mm/atm),
- \( P \) is the partial pressure of the gas (in atm).
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