For the reversible reaction, N_{2(g)} + 3H_{2 | vedclass

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(D) The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n}$.For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g

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$\frac{1.44 	imes 10^{-5}}{(0.082 	imes 773)^{-2}}$

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(D) The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n}$.For the reaction $N_{2(g)} + 3H_{2(g)} ightleftharpoons 2NH_{3(g)}$, the change in moles of gas is $\Delta n = n_p - n_r = 2 - (1 + 3) = -2$.The temperature $T = 500 + 273 = 773 	ext{ K}$.The gas constant $R = 0.082 	ext{ L atm K}^{-1} 	ext{ mol}^{-1}$.Substituting these values into the formula: $K_p = K_c(RT)^{-2}$.Rearranging for $K_c$, we get $K_c = \frac{K_p}{(RT)^{-2}}$.Substituting the given $K_p$ value: $K_c = \frac{1.44 	imes 10^{-5}}{(0.082 	imes 773)^{-2}}$.

For the reversible reaction, $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$. When the partial pressure is measured in atmosphere, the value of $K_p$ at $500^{\circ}\text{C}$ is $1.44 \times 10^{-5}$. The value of $K_c$ when the concentration is expressed in $\text{mol L}^{-1}$ is:

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