9.2 g of N2O4(g) is placed in a closed 1-litre vessel and heated until equilibrium is reached: N2O4(g) ⇌ 2NO2(g). At equilibrium, 50% of N2O4 has dissociated. What is the equilibrium constant Kc (in mol/L)? [Molar mass of N2O4 = 92 g/mol]

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Accepted Answer

0.2. Initial moles N2O4 = 9.2/92 = 0.1 mol in 1 L. At 50% dissociation: N2O4 reacted = 0.05 mol; N2O4 remaining = 0.05 mol; NO2 formed = 2*0.05 = 0.10 mol. Concentrations in 1 L: [N2O4] = 0.05 M, [NO2] = 0.10 M. Kc = [NO2]²/[N2O4] = (0.10)²/(0.05) = 0.01/0.05 = 0.2 mol/L.

9.2 g of N2O4(g) is placed in a closed 1-litre vessel and heated until equilibrium is reached: N2O4(g) ⇌ 2NO2(g). At equilibrium, 50% of N2O4 has dissociated. What is the equilibrium constant Kc (in mol/L)? [Molar mass of N2O4 = 92 g/mol]

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