Quiz 3 Question 4C

[Alisha Clark]

If delta G is positive, why would the forward reaction occur faster than the reverse reaction?

[Jessica Manzano 1B]

My quiz is a different version, but I'm referencing my quiz question that looks the most relevant to your question.

The reaction coordinate diagram illustrates two peaks, indicating that the reaction has two steps. The forward reaction occurs faster because the first step in the forward reaction requires a smaller activation energy, which is indicated by the smaller peak. Reactants of the forward reaction will move past their step 1 faster than the reactants of the reverse reaction will move past their step 1, the higher peak. Additionally, the forward reaction is exergonic, meaning it is more favorable than the reverse reaction, which is endergonic.