Solid `NH_(4)HS(s)` (ammonium hydrogen sulphate) dissociates to give `NH_(3)(g)` and `H_(2)S(g)` and is allowed to attain equilibrium at `100^(@)C`. If the value of `K_(p)` for its dissociation is found to be `0.34`, find the total pressure at equilibrium at `100^(@)C`. If the value of `K_(p)` for its dissociation is found to be `0.34`, find the total pressure at equilibrium and partical pressure of each component.

Explanation

To solve the problem, we will follow these steps:

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

### Step 2: Define the changes in concentration
Let’s assume that initially we have 1 mole of NH₄HS. At equilibrium, let \( x \) moles of NH₃ and \( x \) moles of H₂S be produced. Therefore, at equilibrium:
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