The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Is each of the following statements true or false? (b) For both paths, the rate of the reverse reaction is slower than the rate of the forward reaction.

Video transcript

Hello everyone today. We have the following question. Hypothetical reaction can have two possible pathways as the same at the same temperature as shown below. Which statement is true for both paths. So for both of these reactions, the difference and our potential energy between the products down here. So we have our products down here and the activated complex. These two lines there is going to be greater than the difference between the potential energy of the reactant and the activated complex. So the potential energy of the products and the activated complex is going to be greater than the potential energy of the reactant, which is up here and the activated complex. This means that the activation energy overall for the reverse reaction. So the activation energy for the reverse reaction is going to be greater than the activation energy for the forward reaction. Ultimately a higher activation energy indicates a slow rate of reaction. It is an inverse relationship. And so that's going to make answer choice. A are correct answer. The rate of the forward reaction is faster than the rate of the reverse reaction. And so with that we've answered the question. I hope this helped. And until next time.