Which of the following statements about catalysts is false? A catalyst provides a different reaction pathway with a lower activation energy. A catalyst cannot affect the overall energy change for the reaction. A catalyst speeds up both the forward and reverse reactions. A catalyst is present before the reaction begins, and is also present in the same form after the reaction ends. A catalyst stabilizes the product of the reaction relative to the reactant.

We can answer this question by looking at a plot of Energy vs. Reaction Progress (attached) for a reaction without a catalyst (black line) and the same reaction with a catalyst (orange line).

A catalyst provides a different reaction pathway with a lower activation energy. TRUE. The catalyzed reaction has a transition state with a lower activation energy.

A catalyst cannot affect the overall energy change for the reaction. TRUE. The overall energy change (ΔH) is the same in both cases.

A catalyst speeds up both the forward and reverse reactions. TRUE. This is the reason why catalysts do not affect the equilibrium. They increase direct and inverse reaction rates.

A catalyst is present before the reaction begins, and is also present in the same form after the reaction ends. TRUE. This is a key difference between reactants and catalysts. Catalysts can be recovered unaltered at the end of the reaction.

A catalyst stabilizes the product of the reaction relative to the reactant. FALSE. A catalyst stabilizes the transition state by decreasing the activation energy.