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title: "The initial rates of the reaction represented by the equation below were measured in three separate trials at \\(298 \\text{ K}\\).  \\[ 2\\text{NO}_2(g) + \\text{F}_2(g) \\rightarrow 2\\text{NO}_2\\text{F}(g) \\]  | Trial | \\([\\text{NO}_2]\\ (\\text{M})\\) | \\([\\text{F}_2]\\ (\\text{M})\\) | Initial Rate of Formation of \\(\\text{NO}_2\\text{F}\\ (\\text{M}\\cdot\\text{s}^{-1})\\) | | :—: | :—: | :—: | :—: | | 1 | \\(0.10\\) | \\(0.10\\) | \\(2.0 \\times 10^{-4}\\) | | 2 | \\(0.20\\) | \\(0.10\\) | \\(4.0 \\times 10^{-4}\\) | | 3 | \\(0.20\\) | \\(0.30\\) | \\(1.2 \\times 10^{-3}\\) |  Based on the data in the table, which of the following is the correct rate law and overall reaction order for the reaction?"
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url: "https://nerd-notes.com/ubq/119667/"
date_modified: "2026-08-21T08:11:59+00:00"
---

# The initial rates of the reaction represented by the equation below were measured in three separate trials at \(298 \text{ K}\).

\[ 2\text{NO}_2(g) + \text{F}_2(g) \rightarrow 2\text{NO}_2\text{F}(g) \]

| Trial | \([\text{NO}_2]\ (\text{M})\) | \([\text{F}_2]\ (\text{M})\) | Initial Rate of Formation of \(\text{NO}_2\text{F}\ (\text{M}\cdot\text{s}^{-1})\) |
| :—: | :—: | :—: | :—: |
| 1 | \(0.10\) | \(0.10\) | \(2.0 \times 10^{-4}\) |
| 2 | \(0.20\) | \(0.10\) | \(4.0 \times 10^{-4}\) |
| 3 | \(0.20\) | \(0.30\) | \(1.2 \times 10^{-3}\) |

Based on the data in the table, which of the following is the correct rate law and overall reaction order for the reaction?

The initial rates of the reaction represented by the equation below were measured in three separate trials at \(298 \text{ K}\).

\[ 2\text{NO}_2(g) + \text{F}_2(g) \rightarrow 2\text{NO}_2\text{F}(g) \]

| Trial | \([\text{NO}_2]\ (\text{M})\) | \([\text{F}_2]\ (\text{M})\) | Initial Rate of Formation of \(\text{NO}_2\text{F}\ (\text{M}\cdot\text{s}^{-1})\) |
| :---: | :---: | :---: | :---: |
| 1 | \(0.10\) | \(0.10\) | \(2.0 \times 10^{-4}\) |
| 2 | \(0.20\) | \(0.10\) | \(4.0 \times 10^{-4}\) |
| 3 | \(0.20\) | \(0.30\) | \(1.2 \times 10^{-3}\) |

Based on the data in the table, which of the following is the correct rate law and overall reaction order for the reaction?

- **A.** \(\text{Rate} = k[\text{NO}_2]^2[\text{F}_2]\), and the reaction is third order overall.
- **B.** \(\text{Rate} = k[\text{NO}_2]^2[\text{F}_2]^2\), and the reaction is fourth order overall.
- **C.** \(\text{Rate} = k[\text{NO}_2][\text{F}_2]^2\), and the reaction is third order overall.
- **D.** \(\text{Rate} = k[\text{NO}_2][\text{F}_2]\), and the reaction is second order overall.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119667/*