For the equilibrium: `NH_4HS(s) = NH_3(g) + H_2S(g), K_p = 0.05 atm^2 ` at `20^@C`. If 0.06 role of solid `NH_4 HS` is placed in a 2.40-litre flask at `20^@C` , calculate the percentage of the solid decomposed under equilibrium.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Write the equilibrium expression for the reaction.
The equilibrium reaction is:
\[ \text{NH}_4\text{HS}(s) \rightleftharpoons \text{NH}_3(g) + \text{H}_2\text{S}(g) \]

The equilibrium constant \( K_p \) is given by:
\[ K_p = \frac{P_{\text{NH}_3} \cdot P_{\text{H}_2\text{S}}}{1} \]
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