A `100 dm^(3)` flask contains `10 mol` each of `N_(2)` and `H_(2)` at `700 K`. After equilibrium was reached, partial pressure of `H_(2)` was `1 atm`. At this point, `5 L` of `H_(2)O(l)` was injected and gas mixture was cooled to `298 K`. Find out the gas pressure.

Explanation

To solve the problem step-by-step, let's break it down into manageable parts.

### Step 1: Determine Initial Conditions
We start with a 100 dm³ flask containing 10 moles each of \(N_2\) and \(H_2\) at 700 K.

### Step 2: Calculate the Partial Pressure of \(H_2\)
Using the ideal gas law, we can calculate the partial pressure of \(H_2\) at equilibrium:
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