Dry air contains 79% `N_(2)` and 21% `O_(2)` . Determine the proportion of `N_(2)` and `O_(2)` ( in terms of mole fractions) dissolved in water at 1 atm pressure . Henry's law constant for `N_(2)` and `O_(2)` in `H_(2)O` are `8.54 xx 10^(4)` atm and `4.56 xx 10^(4) ` atm respectively.

Explanation

To solve the problem of determining the mole fractions of nitrogen (N₂) and oxygen (O₂) dissolved in water at 1 atm pressure, we will use Henry's law, which states that the concentration of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. The formula for Henry's law is given by:

\[ P_{gas} = K_H \times X_{gas} \]

Where:
- \( P_{gas} \) is the partial pressure of the gas,
- \( K_H \) is Henry's law constant for the gas,
- \( X_{gas} \) is the mole fraction of the gas in the liquid.
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