The accompanying diagram,which describes the fate of the intermediate in a reversible reaction,implies that:

Question

Quizplus · Accepted Answer

The diagram shows that the intermediate can form both product A and product B. However, product B is more stable than product A, as it is located at a lower energy level. Therefore, according to the principle of microscopic reversibility, the formation of the more stable product (B) will be favored in the reverse reaction. This also implies that the more stable product (B) will form more rapidly in the forward reaction. Therefore, choice B is the best answer.

The Accompanying Diagram,which Describes the Fate of the Intermediate in a Reversible