The Kp of the reaction is `NH_4HS(s)⇌NH_3(g)+H_2S( g)`. If the total pressure at equilibrium is 42 atm.

Explanation

To solve the problem, we need to calculate the equilibrium constant \( K_p \) for the reaction:

\[ \text{NH}_4\text{HS}(s) \rightleftharpoons \text{NH}_3(g) + \text{H}_2\text{S}(g) \]

Given that the total pressure at equilibrium is 42 atm, we can follow these steps:

### Step 1: Set up the equilibrium expression
At equilibrium, the partial pressures of the gases can be represented as follows:
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