The equilibrium constant for a reaction is related to the rate constants for the reaction as follows:

Question

Quizplus · Accepted Answer

The equilibrium constant is defined as the ratio of product concentrations to reactant concentrations raised to their respective stoichiometric coefficients. For a generic reaction:
aA + bB ↔ cC + dD
The equilibrium constant is:
Kc = [C]^c[D]^d/[A]^a[B]^b
The rate law for the forward reaction is:
Ratef = kforward[A]^a[B]^b
The rate law for the reverse reaction is:
Rater = kreverse[C]^c[D]^d
At equilibrium, the rates are equal:
Ratef = Rater
Substituting in the rate laws and rearranging gives to choice B:
Kc = [C]^c[D]^d/[A]^a[B]^b = kforward/kreverse

The Equilibrium Constant for a Reaction Is Related to the Rate