For the reaction 2 HI_{(g)} rightleftharpoon | vedclass

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(A) The given reaction is $2 \ HI_{(g)} \rightleftharpoons H_{2(g)} + I_{2(g)} - Q \ kJ$. For this reaction,the change in the number of moles of gaseo

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temperature

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(A) The given reaction is $2 \ HI_{(g)} \rightleftharpoons H_{2(g)} + I_{2(g)} - Q \ kJ$. For this reaction,the change in the number of moles of gaseous species is $\Delta n_g = n_p - n_R = 2 - 2 = 0$. Since $\Delta n_g = 0$,the equilibrium constant is not affected by changes in pressure or volume. $A$ catalyst only speeds up the attainment of equilibrium and does not alter the value of the equilibrium constant. The equilibrium constant ($K_c$ or $K_p$) is a function of temperature only,as described by the van't Hoff equation. Therefore,for this reaction,the equilibrium constant depends only upon the temperature.

For the reaction $2 \ HI_{(g)} \rightleftharpoons H_{2(g)} + I_{2(g)} - Q \ kJ$,the equilibrium constant depends upon

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