For which of the following reactions is K_c l | vedclass

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(D) The relationship between $K_p$ and $K_c$ is given by the equation $K_p = K_c(RT)^{\Delta n_g}$,where $\Delta n_g$ is the change in the number of m

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$H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$

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(D) The relationship between $K_p$ and $K_c$ is given by the equation $K_p = K_c(RT)^{\Delta n_g}$,where $\Delta n_g$ is the change in the number of moles of gaseous products and reactants.For $K_c \leq K_p$,we must have $\Delta n_g \geq 0$.$(A)$ $\Delta n_g = 2 - 3 = -1$. Since $\Delta n_g $(B)$ $\Delta n_g = 2 - (1 + 3) = -2$. Since $\Delta n_g $(C)$ $\Delta n_g = 2 - (1 + 2) = -1$. Since $\Delta n_g $(D)$ $\Delta n_g = 2 - (1 + 1) = 0$. Since $\Delta n_g = 0$,$K_p = K_c(RT)^0 = K_c$. Thus,$K_c = K_p$ satisfies the condition $K_c \leq K_p$.

For which of the following reactions is $K_c \leq K_p$ at $298 \ K$?

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