A definite amount of solid `NH_(4)HS` is placed in a flask aleady containing ammoina gas at a certain temperature and `0.50` atm pressure. `NH_(4)HS` decomposes to give `NH_(3)` and `H_(2)S` and at equilibrium total pressure in flask is `0.84` atm. The equilibrium constant for the reaction is:

Explanation

To determine the equilibrium constant for the decomposition of solid `NH₄HS` into ammonia (`NH₃`) and hydrogen sulfide (`H₂S`), we can follow these steps:

### Step 1: Write the balanced chemical equation
The decomposition reaction of ammonium hydrogen sulfide can be represented as:
\[ \text{NH}_4\text{HS (s)} \rightleftharpoons \text{NH}_3 \text{ (g)} + \text{H}_2\text{S (g)} \]

### Step 2: Identify initial conditions
Initially, we have:
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