Value of \(K_P\) for the equilibrium reaction
\(\mathrm{N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}}\) at 288 K is 47.9. The \(K_C\) for this reaction at same temperature is ____________. (Nearest integer)
(R = 0.083 L bar \(\mathrm{K^{-1}\,mol^{-1}}\))
\(\mathrm{N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}}\) at 288 K is 47.9. The \(K_C\) for this reaction at same temperature is ____________. (Nearest integer)
(R = 0.083 L bar \(\mathrm{K^{-1}\,mol^{-1}}\))
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Correct Answer: 2
Solution and Explanation
\(K_p = K_c\,(RT)^{\Delta n_g}\), so \(K_c = \dfrac{K_p}{RT}\)
\(RT = 0.083\times 288 = 23.904\)
\(K_c = \dfrac{47.9}{23.904} = 2.004 \approx 2\)
Answer: 2
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