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(A) 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

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$N_2(g) + O_2(g) \rightleftharpoons 2NO(g)$

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(A) 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 $K_p = K_c$, the condition is $\Delta n_g = 0$.Let us calculate $\Delta n_g$ for each reaction:$(A)$ $N_2(g) + O_2(g) \rightleftharpoons 2NO(g) \implies \Delta n_g = 2 - (1+1) = 0$.$(B)$ $H_2O(g) + CO(g) \rightleftharpoons H_2(g) + CO_2(g) \implies \Delta n_g = (1+1) - (1+1) = 0$.$(C)$ $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \implies \Delta n_g = 2 - (1+3) = -2$.$(D)$ $H_2(g) + I_2(g) \rightleftharpoons 2HI(g) \implies \Delta n_g = 2 - (1+1) = 0$.Reactions $(A)$, $(B)$, and $(D)$ all satisfy the condition $\Delta n_g = 0$. In standard chemistry problems of this type, if multiple options are correct, the question may be flawed or require selecting the most representative example.

Given below are certain reactions. Identify the reaction for which $K_p = K_c$.

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For the reaction: $H_{2(g)} + CO_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$,if the initial concentration of $[H_2] = [CO_2] = 1 \ M$ and $x \ mol/L$ of hydrogen is consumed at equilibrium,the correct expression for $K_c$ is:

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