An amount of solid NH4HS is placed in a flask already containing ammonia gas at a certain temperature and pressure of0.50 atm. Ammonium hydrogen sulphide decomposes to yield NH3 and H2S gasses in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 0.84 atm. The equilibrium constant for NH4HS decomposition at this temperature is

An amount of solid ${NH}_{4} HS$ is placed in a flask already containing ammonia gas at a certain temperature and pressure of0.50 atm. Ammonium hydrogen sulphide decomposes to yield ${NH}_{3}$ and $H_{2} S$ gasses in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 0.84 atm. The equilibrium constant for ${NH}_{4} HS$ decomposition at this temperature is

A
$0.17 {atm}^{2}$
B
$0.11 {atm}^{2}$
C
$0.30 {atm}^{2}$
D
$0.18 {atm}^{2}$

Solution:

We have ${NH}_{4} HS (s) ⇌ {NH}_{3} (g) + H_{2} S (g)$

$\begin{array}{l} t & 0.5 atm \\ t_{eq} & 0.50 atm + p p \end{array}$

We are given that $p_{eq} = 0.84 atm = (0.50 atm + p) + p$

This gives p = 0.17 atm

Hence

$K_{p} = (0.5 atm + 0.17 atm) (0.17 atm) = 0.1139 {atm}^{2}$

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