Consider the reaction
\(\mathrm{N_2O_4(g)} \rightleftharpoons 2\mathrm{NO_2(g)}\)
The temperature at which \(K_C = 20.4\) and \(K_P = 600.1\), is ____________ K. (Round off to the Nearest Integer). [Assume all gases are ideal and \(R = 0.0831\ \mathrm{L\ bar\ K^{-1}\ mol^{-1}}\)]
\(\mathrm{N_2O_4(g)} \rightleftharpoons 2\mathrm{NO_2(g)}\)
The temperature at which \(K_C = 20.4\) and \(K_P = 600.1\), is ____________ K. (Round off to the Nearest Integer). [Assume all gases are ideal and \(R = 0.0831\ \mathrm{L\ bar\ K^{-1}\ mol^{-1}}\)]
Show Hint
Correct Answer: 354
Solution and Explanation
\(K_P = K_C (RT)^{1}\), so \(T = \frac{K_P}{K_C R} = \frac{600.1}{20.4 \times 0.0831}\).
\(20.4 \times 0.0831 = 1.6952\), so \(T = 600.1/1.6952 = 353.99 \approx 354\ \mathrm{K}\).
Answer: 354
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