At `25^@C` the equilibrium constant for the reaction `NH_(4)SH(s) Leftrightarrow NH_(5)(g)+H_(2)S(g)`
is `K_(p)=12`. A 10-0 litre flask is charged with 1 atm of pure `NH_(3) (g)" at "25^@C`. What is the minimum mass in grams of `NH_(4)HS` that must be added to the flask in order to acheive equilibrium?

Explanation

To solve the problem step-by-step, we need to analyze the given reaction and the conditions provided.

### Step 1: Write the balanced chemical equation
The reaction is given as:
\[ \text{NH}_4\text{SH}(s) \rightleftharpoons \text{NH}_3(g) + \text{H}_2\text{S}(g) \]

### Step 2: Identify the initial conditions
We start with a 10.0 L flask charged with 1 atm of pure \( \text{NH}_3(g) \) at 25°C.
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