(C) For the given reaction,$A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$,the change in the number of moles of gaseous species is $\Delta n_

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(C) For the given reaction,$A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$,the change in the number of moles of gaseous species is $\Delta n_g = (1 + 1) - (1 + 1) = 0$.Since $\Delta n_g = 0$,the pressure change does not affect the equilibrium position or the equilibrium constant.The equilibrium constant $K_c$ is a function of temperature only.Therefore,increasing the pressure will not disturb the equilibrium constant.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Le-Chaterlier principle and It’s application

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For the reaction,$A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$; $\Delta H = Q \ kJ$,the equilibrium constant cannot be disturbed by

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A
addition of $A$
B
addition of $D$
C
increasing of pressure
D
increasing of temperature

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6-1.Equilibrium (Chemical Equilibrium)

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Le-Chaterlier principle and It’s application

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For the reaction,$A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$; $\Delta H = Q \ kJ$,the equilibrium constant cannot be disturbed by

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In what manner will an increase of pressure affect the following equilibrium equation?
$C_{(s)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2(g)}$