`N_(2)``O_(4)` is `25%` dissociated at `37^(@)C` and one atmosphere pressure. Calculate (i) `K_(p)` and (ii) the percentage dissociation at 0.1 atm and `37^(@)C`

Explanation

To solve the problem, we will follow these steps:

### Step 1: Write the balanced chemical equation
The dissociation of dinitrogen tetroxide (N₂O₄) can be represented as:
\[ N_2O_4(g) \rightleftharpoons 2NO_2(g) \]

### Step 2: Define the initial conditions
At the start, we assume we have 1 mole of N₂O₄. Given that it is 25% dissociated at equilibrium, we can define:
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