---
title: "The reaction between nitrogen dioxide and fluorine gas is represented by the following balanced equation.  \\[ 2\\,\\text{NO}_2(g) + \\text{F}_2(g) \\rightarrow 2\\,\\text{NO}_2\\text{F}(g) \\]  A proposed two-step mechanism for the reaction is shown below.  \\[ \\text{Step 1: } \\text{NO}_2(g) + \\text{F}_2(g) \\rightarrow \\text{NO}_2\\text{F}(g) + \\text{F}(g) \\quad (\\text{slow}) \\]  \\[ \\text{Step 2: } \\text{NO}_2(g) + \\text{F}(g) \\rightarrow \\text{NO}_2\\text{F}(g) \\quad (\\text{fast}) \\]  Based on the proposed mechanism, which of the following predicts the factor by which the initial rate of the reaction will change if the initial concentration of \\(\\text{NO}_2(g)\\) is doubled while the initial concentration of \\(\\text{F}_2(g)\\) remains constant, and correctly identifies an intermediate in the reaction?"
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/121513/"
date_modified: "2026-08-23T05:04:58+00:00"
---

# The reaction between nitrogen dioxide and fluorine gas is represented by the following balanced equation.

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

A proposed two-step mechanism for the reaction is shown below.

\[ \text{Step 1: } \text{NO}_2(g) + \text{F}_2(g) \rightarrow \text{NO}_2\text{F}(g) + \text{F}(g) \quad (\text{slow}) \]

\[ \text{Step 2: } \text{NO}_2(g) + \text{F}(g) \rightarrow \text{NO}_2\text{F}(g) \quad (\text{fast}) \]

Based on the proposed mechanism, which of the following predicts the factor by which the initial rate of the reaction will change if the initial concentration of \(\text{NO}_2(g)\) is doubled while the initial concentration of \(\text{F}_2(g)\) remains constant, and correctly identifies an intermediate in the reaction?

The reaction between nitrogen dioxide and fluorine gas is represented by the following balanced equation.

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

A proposed two-step mechanism for the reaction is shown below.

\[ \text{Step 1: } \text{NO}_2(g) + \text{F}_2(g) \rightarrow \text{NO}_2\text{F}(g) + \text{F}(g) \quad (\text{slow}) \]

\[ \text{Step 2: } \text{NO}_2(g) + \text{F}(g) \rightarrow \text{NO}_2\text{F}(g) \quad (\text{fast}) \]

Based on the proposed mechanism, which of the following predicts the factor by which the initial rate of the reaction will change if the initial concentration of \(\text{NO}_2(g)\) is doubled while the initial concentration of \(\text{F}_2(g)\) remains constant, and correctly identifies an intermediate in the reaction?

- **A.** The initial rate will increase by a factor of \(4\), because \(\text{NO}_2(g)\) has a stoichiometric coefficient of \(2\) in the overall balanced chemical equation, and \(\text{NO}_2\text{F}(g)\) is an intermediate.
- **B.** The initial rate will increase by a factor of \(4\), because two molecules of \(\text{NO}_2(g)\) are consumed across the steps of the mechanism, and \(\text{F}(g)\) is an intermediate.
- **C.** The initial rate will increase by a factor of \(2\), because the rate law determined by the slow step is \(\text{Rate} = k[\text{NO}_2][\text{F}_2]\), and \(\text{F}(g)\) is an intermediate.
- **D.** The initial rate will increase by a factor of \(2\), because the rate law determined by the slow step is \(\text{Rate} = k[\text{NO}_2][\text{F}_2]\), and \(\text{NO}_2\text{F}(g)\) is an intermediate.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121513/*