Consider the equilibrium 2 NOCl(g) ⇄ NO(g) + CL₂ (g).At 800.0 K, the equilibrium constant is approximately 6.1 * 10^-8.Which statement below about this equilibrium is true?

Question

Quizplus · Accepted Answer

The equilibrium constant (K) being a specific value (approximately 6.1 x 10^-8 at 800.0 K) indicates that at equilibrium, the rate of the forward reaction (kf) equals the rate of the reverse reaction (kr). However, for K to be less than 1, as it is in this case, it suggests that the concentration of reactants is higher than that of products at equilibrium, implying that the reverse reaction is favored. This does not mean kf < kr at equilibrium (they are equal at equilibrium); rather, it suggests that initially, before equilibrium is reached, the forward reaction rate must have been less than the reverse reaction rate for the system to adjust to this equilibrium state. The correct interpretation of the given equilibrium constant value is that it reflects the ratio of product to reactant concentrations at equilibrium, not directly the rates of the forward and reverse reactions.

Consider the Equilibrium 2 NOCl(g) ⇄ NO(g) + CL2 (G)

Consider the Equilibrium 2 NOCl(g) ⇄ NO(g) + CL₂ (G)