If `N_(2)` gas is bubbled through water at `293 K`, how many millimoles of `N_(2)` gas would dissolve in`1 L` of water. Assume that` N_(2)` exerts a partial pressure of 0.987 bar. Given that Henry law constant for `N_(2)` at `293 K` is 76.48 kbar.

Explanation

To solve the problem of how many millimoles of \( N_2 \) gas would dissolve in 1 L of water at 293 K with a partial pressure of 0.987 bar, we can use Henry's Law. Here’s a step-by-step breakdown of the solution:

### Step 1: Write down the known values
- Partial pressure of \( N_2 \) gas, \( p_{N_2} = 0.987 \, \text{bar} \)
- Henry's Law constant for \( N_2 \) at 293 K, \( k_H = 76.48 \, \text{kbar} = 76480 \, \text{bar} \)

### Step 2: Use Henry's Law to find the mole fraction of \( N_2 \)
According to Henry's Law, the mole fraction \( x_{N_2} \) of the gas in the solution can be calculated using the formula:
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