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An amount of solid ${NH}_{4} HS$ is placed in a flask already containing ammonia gas at a certain temperature and 0.50atm pressure. Ammonium hydrogen sulphide decomposes to yield ${NH}_{3}$ and $H_{2} S$ gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 0.84atm ? The equilibrium constant for ${NH}_{4} HS$ decomposition at this temperature is:

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0.17

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detailed solution

Correct option is A

The reaction process as;

$\begin{aligned} {NH}_{4} HS ⇌ {NH}_{3} + H_{2} S \\ 0.5 + P P \end{aligned}$

Here pressure

$P = 0.5 + P + P$

$P = 0.5 + 2 P = 0.84$

$K_{P} = P_{{NH}_{3}} \times P_{H_{2} s}$

$K_{P} = 0.67 \times 0.17$

$K_{P} = 0.1139$

Thus, the correct option is A.

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