## K

eq [A]a [B]b [C]c where brackets denote the concentrations of the molecules. The rate of the forward reaction (left to right in Equation 2-1) is

Rateforward = kf[A]a[B]b[C]c where kf is the rate constant for the forward reaction. Similarly, the rate of the reverse reaction (right to left in Equation 2-1) is

Rater

Ar[X]x[Y]y[Z]z where kr is the rate constant for the reverse reaction. At equilibrium the forward and reverse rates are equal, so Rateforward/Ratereverse = 1. By rearranging these equations, we can express the equilibrium constant as the ratio of the rate constants

eq k

0 0

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