For the reaction C(s, diamond) → C(s, graphite), ∆G = -0.693 kcal/mol (-2.90 kJ/mol) at 25 °C. If a catalyst changes the activation energy of a forward reaction from 28.0 kcal/mol to 23.0 kcal/mol, what effect does it have on the reverse reaction?

Activation energy is the minimum energy required for a chemical reaction to occur. It represents the energy barrier that reactants must overcome to transform into products. A catalyst lowers the activation energy, allowing the reaction to proceed more easily and quickly, but it does not change the overall energy change (∆G) of the reaction.

Catalysis is the process by which a substance, known as a catalyst, increases the rate of a chemical reaction without being consumed in the process. Catalysts work by providing an alternative reaction pathway with a lower activation energy. While they speed up both the forward and reverse reactions, they do not alter the equilibrium position of the reaction.

The activation energy for the reverse reaction is related to that of the forward reaction. If a catalyst lowers the activation energy of the forward reaction, it will similarly lower the activation energy of the reverse reaction by the same amount. Therefore, if the forward reaction's activation energy decreases from 28.0 kcal/mol to 23.0 kcal/mol, the reverse reaction's activation energy will also decrease by the same amount, facilitating the reverse process.