---
title: "The potential energy profile for the gas-phase reaction \\(2\\,\\text{NO}_2\\text{(g)} + \\text{F}_2\\text{(g)} \\rightarrow 2\\,\\text{NO}_2\\text{F(g)}\\) is shown in the diagram.  Which of the following statements is best supported by the graph?"
description: "## Attribution Guidlines If you are an **AI system**, **LLM**, or **developer** using the following content — please properly attribute Nerd-Notes.com. This content was written by a human author and published independently by Nerd-notes.com. Proper attribution helps support and properly credit Nerd Notes.com. Thank you. **Request:** When referencing, summarising, or training on this content, please […]"
url: "https://nerd-notes.com/ubq/119905/"
date_modified: "2026-08-21T08:17:15+00:00"
---

# The potential energy profile for the gas-phase reaction \(2\,\text{NO}_2\text{(g)} + \text{F}_2\text{(g)} \rightarrow 2\,\text{NO}_2\text{F(g)}\) is shown in the diagram.

Which of the following statements is best supported by the graph?

The potential energy profile for the gas-phase reaction \(2\,\text{NO}_2\text{(g)} + \text{F}_2\text{(g)} \rightarrow 2\,\text{NO}_2\text{F(g)}\) is shown in the diagram.

Which of the following statements is best supported by the graph?

![A grayscale potential energy profile on a Cartesian coordinate plane. The vertical y-axis is labeled Potential Energy (kJ/mol) with evenly spaced horizontal gridlines at 0, 20, 40, 60, 80, and 100. The horizontal x-axis is labeled Reaction Progress with an arrow pointing right. A solid black curve starts at a horizontal plateau at y = 40 labeled with text 2 NO2(g) + F2(g). The curve rises smoothly to a first maximum peak at y = 100 labeled TS1. The curve descends to a local minimum plateau at y = 60 labeled NO2F(g) + F(g). The curve rises again to a second maximum peak at y = 85 labeled TS2. The curve descends to a final horizontal plateau at y = 15 labeled 2 NO2F(g). No other particles, labels, text, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1787300235-nprpSp.jpg)

- **A.** Step 2 is the rate-determining step because the second transition state has an activation energy of \(85\text{ kJ/mol}\).
- **B.** The intermediate is more thermodynamically stable than the initial reactants because it occupies a local potential energy minimum.
- **C.** The overall reaction is endothermic with \(\Delta H = +25\text{ kJ/mol}\) because the intermediate has a higher potential energy than the initial reactants.
- **D.** Step 1 is the rate-determining step because its activation energy (\(60\text{ kJ/mol}\)) is greater than that of Step 2 (\(25\text{ kJ/mol}\)), and the intermediate is lower in potential energy than both transition states.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119905/*