Consider the reaction N2O4(g) ⇌ 2NO2(g). The temperature at which Kc = 20.4 and Kp = 600.1, is ______ K. (Round off to the nearest integer).
[Assume all gases are ideal and R = 0.0831 L bar mol⁻¹ K⁻¹]
Consider the reaction N2O4(g) ⇌ 2NO2(g). The temperature at which Kc = 20.4 and Kp = 600.1, is ______ K. (Round off to the nearest integer).
[Assume all gases are ideal and R = 0.0831 L bar mol⁻¹ K⁻¹]
The reaction is N? O? (g)? 2NO? (g).
Δn_g = (moles of gaseous products) - (moles of gaseous reactants) = 2 - 1 = 1.
The relationship between Kp and Kc is Kp = Kc (RT)^Δn_g.
600.1 = 20.4 * (0.0831 * T)¹
T = 600.1 / (20.4 * 0.0831) = 353.99 K.
The answer, rounded off, is 354 K.
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