---
title: "The potential energy profiles for the aqueous hydrolysis of an ester in the presence and absence of an acid catalyst are shown in the diagram below.  \\[ \\text{CH}_3\\text{COOCH}_3\\text{(aq)} + \\text{H}_2\\text{O(l)} \\rightarrow \\text{CH}_3\\text{COOH(aq)} + \\text{CH}_3\\text{OH(aq)} \\]  Which of the following statements is best supported by the reaction energy profiles?"
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url: "https://nerd-notes.com/ubq/123688/"
date_modified: "2026-09-28T12:01:59+00:00"
---

# The potential energy profiles for the aqueous hydrolysis of an ester in the presence and absence of an acid catalyst are shown in the diagram below.

\[ \text{CH}_3\text{COOCH}_3\text{(aq)} + \text{H}_2\text{O(l)} \rightarrow \text{CH}_3\text{COOH(aq)} + \text{CH}_3\text{OH(aq)} \]

Which of the following statements is best supported by the reaction energy profiles?

The potential energy profiles for the aqueous hydrolysis of an ester in the presence and absence of an acid catalyst are shown in the diagram below.

\[ \text{CH}_3\text{COOCH}_3\text{(aq)} + \text{H}_2\text{O(l)} \rightarrow \text{CH}_3\text{COOH(aq)} + \text{CH}_3\text{OH(aq)} \]

Which of the following statements is best supported by the reaction energy profiles?

![A reaction energy profile graph plotted on bare axes without gridlines. The vertical axis is labeled Potential Energy (kJ/mol) and the horizontal axis is labeled Reaction Coordinate. A flat horizontal plateau at 20 kJ/mol represents the reactants, and a flat horizontal plateau at 0 kJ/mol represents the products. A solid black curve labeled Uncatalyzed pathway rises from 20 kJ/mol to a single smooth peak at 100 kJ/mol before descending to 0 kJ/mol. A dashed black curve labeled Catalyzed pathway starts at 20 kJ/mol, rises to a first peak at 55 kJ/mol, dips to a shallow local minimum at 35 kJ/mol, rises to a second peak at 60 kJ/mol, and descends to 0 kJ/mol. No other lines, labels, shaded regions, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1790596919-pCwSuA.jpg)

- **A.** The catalyst introduces an alternative two-step pathway involving an intermediate, reducing the overall activation energy barrier without changing \(\Delta H\).
- **B.** The catalyst stabilizes the product molecules relative to the reactants, which makes \(\Delta H\) more negative and accelerates the forward rate.
- **C.** The catalyst increases the average kinetic energy of the reactant molecules, allowing a greater fraction of collisions to overcome the original barrier.
- **D.** The catalyst lowers the activation energy of the forward reaction only, increasing the forward rate while leaving the reverse rate unchanged.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123688/*