(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 6-1.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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Kp and Kc Relationship

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The values of $K_p/K_c$ for the following reactions at $300 \ K$ are respectively (At $300 \ K, RT = 24.62 \ dm^3 \ atm \ mol^{-1}$):
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$(ii) \ N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$
$(iii) \ N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

DifficultJEE MAIN 2019

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For the formation of $NH_3$ from $N_2$ and $H_2$ at $500 \ K$,the concentrations of $N_2, H_2$ and $NH_3$ at equilibrium are $1.5 \times 10^{-2} \ M, 3.0 \times 10^{-2} \ M$ and $1.2 \times 10^{-2} \ M$,respectively. The equilibrium constant for the reverse reaction is

MediumTS EAMCET 2018

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For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + \text{heat}$,which of the following relations is correct?

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For the formation of $NH_3$ from $N_2$ and $H_2$ at $500 \ K$,the concentrations of $N_2, H_2$ and $NH_3$ at equilibrium are $1.5 \times 10^{-2} \ M, 3.0 \times 10^{-2} \ M$ and $1.2 \times 10^{-2} \ M$,respectively. The equilibrium constant for the reverse reaction is

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