Chemistry

The equilibrium constant depends on the difference between forward and reverse activation energies—this difference tells you the overall energy change of the reaction. Since both reactions share the same pre-exponential factor, their rate constants depend only on their activation energies through the Arrhenius equation. The ratio of forward to reverse rate constants directly gives you $K_{eq}$, and you can find it using $\ln K = \frac{E_a^{forward} - E_a^{reverse}}{RT}$.

The equilibrium constant depends on the difference between forward and reverse activation energies—this difference tells you the overall energy change of the reaction. Since both reactions share the same pre-exponential factor, their rate constants depend only on their activation energies through the Arrhenius equation. The ratio of forward to reverse rate constants directly gives you $K_{eq}$, and you can find it using $\ln K = \frac{E_a^{forward} - E_a^{reverse}}{RT}$.