Consider an elementary reversible first-order reaction with forward rate constant and backward rate — Chemical Kinetics Chemistry Question
Question
Consider an elementary reversible first-order reaction $A \rightleftharpoons B$ with forward rate constant $k_f$ and backward rate constant $k_b$. At dynamic equilibrium, how is the thermodynamic equilibrium constant ($K_{eq}$) defined kinetically?
Answer: D
💡 Solution & Explanation
At dynamic equilibrium, the net macroscopic rate is zero, meaning the forward rate strictly equals the reverse rate: $k_f[A]_{eq} = k_b[B]_{eq}$. Rearranging this kinetic equality yields the thermodynamic ratio $K_{eq} = \frac{[B]_{eq}}{[A]_{eq}} = \frac{k_f}{k_b}$.
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