For a reversible reaction (first order in both directions)

$A\stackrel{k_1}{\underset{k_2}{\rightleftharpoons }}B$

${\mathrm{k}}_1$and ${\mathrm{k}}_2$ are the rate constant

If equilibrium constant (K) is greater than unity, then:

activation energy for the forward direction $\left({\mathrm{E}}_{\mathrm{af}}\right)$is greater than activation energy for backward reaction $\left({\mathrm{E}}_{\mathrm{ab}}\right)$·

addition of a catalyst will increase both ${\mathrm{k}}_1$ and ${\mathrm{k}}_2$ by same factor

rate of forward reaction is always greater than rate of backward reaction.

amount of product at equilibrium is greater than the amount of reactant.