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(D) The given reaction is a heterogeneous equilibrium: $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$.According to the law of mass action,th

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No effect on partial pressure of $NH_3$ and $H_2S$

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(D) The given reaction is a heterogeneous equilibrium: $NH_4HS_{(s)} ightleftharpoons NH_{3(g)} + H_2S_{(g)}$.According to the law of mass action,the equilibrium constant $K_p$ is given by $K_p = P_{NH_3} 	imes P_{H_2S}$.Since $NH_4HS$ is a solid,its active mass is considered constant and it does not appear in the equilibrium constant expression.Adding more solid $NH_4HS$ to the system does not change the concentration or partial pressure of the gaseous products as long as some solid remains to maintain equilibrium.Therefore,the partial pressures of $NH_3$ and $H_2S$ remain unchanged,and the total pressure remains constant.

Consider the heterogeneous equilibrium in a closed container:
$NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$
If more $NH_4HS_{(s)}$ is added to the equilibrium,what will be the effect on the system?

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Consider the heterogeneous equilibrium in a closed container:$NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$If more $NH_4HS_{(s)}$ is added to the equilibrium,what will be the effect on the system?