(D) The decomposition reaction is: $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$Initial pressure: $P_{NH_3} = 0.50 \ atm$,$P_{H_2S} = 0 \ a

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(D) The decomposition reaction is: $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$Initial pressure: $P_{NH_3} = 0.50 \ atm$,$P_{H_2S} = 0 \ atm$At equilibrium,let the increase in pressure due to decomposition be $x \ atm$ for each gas.$P_{NH_3} = 0.50 + x$$P_{H_2S} = x$Total pressure $P_T = P_{NH_3} + P_{H_2S} = (0.50 + x) + x = 0.84 \ atm$$0.50 + 2x = 0.84$ $\Rightarrow 2x = 0.34$ $\Rightarrow x = 0.17 \ atm$Equilibrium pressures: $P_{NH_3} = 0.50 + 0.17 = 0.67 \ atm$ and $P_{H_2S} = 0.17 \ atm$$K_p = P_{NH_3} \times P_{H_2S} = 0.67 \times 0.17 = 0.1139 \approx 0.11$

Class 11 Chemistry 1 Equilibrium: Chemical Equilibrium Kp and Kc Relationship

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An amount of solid $NH_4HS$ is placed in a flask already containing ammonia gas at a certain temperature and $0.50 \ atm$ pressure. Ammonium hydrogen sulphide decomposes to yield $NH_3$ and $H_2S$ gases in the flask. When the decomposition reaction reaches equilibrium,the total pressure in the flask rises to $0.84 \ atm$. The equilibrium constant for $NH_4HS$ decomposition at this temperature is

AIEEE 2005 All AIEEE

A
$0.3$
B
$0.18$
C
$0.17$
D
$0.11$

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1 Equilibrium: Chemical Equilibrium

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Kp and Kc Relationship

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