How is the equilibrium constant Kc related to the forward and reverse rate constants for a simple reaction?

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Multiple Choice

How is the equilibrium constant Kc related to the forward and reverse rate constants for a simple reaction?

Explanation:
At equilibrium, the forward and reverse processes occur at the same rate. The forward rate is kf [A]^a [B]^b, and the reverse rate is kr [C]^c [D]^d. Setting these equal gives kf [A]^a [B]^b = kr [C]^c [D]^d. Rearranging yields ([C]^c [D]^d)/([A]^a [B]^b) = kf/kr. But the left-hand side is exactly the expression for the equilibrium constant Kc for this reaction. So Kc equals the forward rate constant divided by the reverse rate constant.

At equilibrium, the forward and reverse processes occur at the same rate. The forward rate is kf [A]^a [B]^b, and the reverse rate is kr [C]^c [D]^d. Setting these equal gives kf [A]^a [B]^b = kr [C]^c [D]^d. Rearranging yields ([C]^c [D]^d)/([A]^a [B]^b) = kf/kr. But the left-hand side is exactly the expression for the equilibrium constant Kc for this reaction. So Kc equals the forward rate constant divided by the reverse rate constant.

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