Chemistry

Chemistry

Problem

For the reaction N₂O₄ (g) ⇌ 2 NO₂ (g) at 298 K, the equilibrium constant is K ≈ 0.80. Describe qualitatively the relative concentrations of N₂O₄ and NO₂ present in the equilibrium mixture.
Intuitive explanation

The equilibrium constant tells you the ratio of products to reactants at balance—here, K=[NO2]2[N2O4]=0.80K = \frac{[\text{NO}_2]^2}{[\text{N}_2\text{O}_4]} = 0.80. Since K<1K < 1, the numerator is smaller than the denominator, meaning the system favors the reactant side. You'll have significantly more N₂O₄ molecules than NO₂ at equilibrium, with the dimer remaining largely intact rather than dissociating into the monomer.

Intuitive explanation

The equilibrium constant tells you the ratio of products to reactants at balance—here, K=[NO2]2[N2O4]=0.80K = \frac{[\text{NO}_2]^2}{[\text{N}_2\text{O}_4]} = 0.80. Since K<1K < 1, the numerator is smaller than the denominator, meaning the system favors the reactant side. You'll have significantly more N₂O₄ molecules than NO₂ at equilibrium, with the dimer remaining largely intact rather than dissociating into the monomer.

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