Assume that the decomposition of N 2 O 5 can be represented as 2N 2 O 5 (g) ⇌ 4NO 2 (g) + O 2 (g) and that at a given temperature of 500 K and pressure of 25.5 atm, the reaction approaches equilibrium

Question

Assume that the decomposition of N 2 O 5 can be represented as 2N 2 O 5 (g) ⇌ 4NO 2 (g) + O 2 (g) and that at a given temperature of 500 K and pressure of 25.5 atm, the reaction approaches equilibrium. At equilibrium, the partial pressure of N 2 O 5 (g) is 0.5 atm. The value of K C (in M 3 ) for the reaction at 500 K is (take R = 0.08 L atm/mol/K)

TestHub · Accepted Answer

Let P O2 = k, so P NO2 = 4k Total pressure = 0.5 + 4k + k = 25.5, so k = 5 atm P NO2 = 20 atm and P O2 = 5 atm K P = (20) 4 (5)/(0.5) 2 = 3.2 × 10 6 atm 3 Δn = 5 - 2 = 3 and RT = (0.08)(500) = 40 L atm/mol K C = K P /(RT) 3 = (3.2 × 10 6 )/(40) 3 = (3.2 × 10 6 )/(6.4 × 10 4 ) K C = 50, written as 0050

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