The values of K_p/K_c for the following react | vedclass

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(B) The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n_g}$,which implies $K_p/K_c = (RT)^{\Delta n_g}$.Given $RT = 24.62 \

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$1, 24.62 \ dm^3 \ atm \ mol^{-1}, 1.65 	imes 10^{-3} \ dm^{-6} \ atm^{-2} \ mol^2$

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(B) The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n_g}$,which implies $K_p/K_c = (RT)^{\Delta n_g}$.Given $RT = 24.62 \ dm^3 \ atm \ mol^{-1}$.For reaction $(i): N_{2(g)} + O_{2(g)} ightleftharpoons 2NO_{(g)}$,$\Delta n_g = 2 - (1+1) = 0$. So,$K_p/K_c = (RT)^0 = 1$.For reaction $(ii): N_2O_{4(g)} ightleftharpoons 2NO_{2(g)}$,$\Delta n_g = 2 - 1 = 1$. So,$K_p/K_c = (RT)^1 = 24.62 \ dm^3 \ atm \ mol^{-1}$.For reaction $(iii): N_{2(g)} + 3H_{2(g)} ightleftharpoons 2NH_{3(g)}$,$\Delta n_g = 2 - (1+3) = -2$. So,$K_p/K_c = (RT)^{-2} = (24.62)^{-2} \approx 1.65 	imes 10^{-3} \ dm^{-6} \ atm^{-2} \ mol^2$.

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The values of $K_p/K_c$ for the following reactions at $300 \ K$ are respectively (At $300 \ K, RT = 24.62 \ dm^3 \ atm \ mol^{-1}$):$(i) \ N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$$(ii) \ N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$$(iii) \ N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$