Air contains `O_(2) and N_(2)` in the ratio of `1:4`. Calculate the ratio of solubilities in terms of mole fraction of `O_(2)` and `N_(2)` dissolved in water at atmospheric pressure and room temperature at which Henry's constant for `O_(2)` and `N_(2)` are `3.30xx10^(7)` torr and `6.60xx10^(7)` torr respectively.

Explanation

To solve the given problem, we need to determine the ratio of solubilities in terms of mole fractions of \(O_2\) and \(N_2\) dissolved in water at atmospheric pressure and room temperature. We are given the Henry's constants for \(O_2\) and \(N_2\) as \(3.30 \times 10^7\) torr and \(6.60 \times 10^7\) torr respectively.

### Step-by-Step Solution:

1. **Determine the Partial Pressures:**
- The ratio of \(O_2\) to \(N_2\) in air is \(1:4\).
- Assume the total pressure is 1 bar.
- Calculate the partial pressure of \(O_2\):
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