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Types of Redox Reactions

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

A

0.11

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B

0.17

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C

0.18

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D

0.30

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Solution

The correct option is A $0.11$
${N H}_{4} H S ⇌ {N H}_{3} (g) + H_{2} S (g)$
$a 0.5$
$a - x 0.5 + x x$
Total\quad pressure $= 0.5 + 2 x = 0.84$
$i e, x = 0.17$
$K_{p} = P_{N H_{3}} \times P_{H_{2} S}$
$= (0.67) (0.17)$
$= 0.1139$

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