---
title: "A reversible reaction is represented by the equation below.  \\[ \\text{N}_2\\text{O}_4(g) \\rightleftharpoons 2\\,\\text{NO}_2(g) \\]  At a constant temperature, the system is initially at equilibrium in a \\(1.0\\text{ L}\\) rigid container. At equilibrium, the concentration of \\(\\text{N}_2\\text{O}_4(g)\\) is \\(0.20\\text{ M}\\) and the concentration of \\(\\text{NO}_2(g)\\) is \\(0.40\\text{ M}\\). The volume of the container is rapidly expanded to \\(2.0\\text{ L}\\) at the same temperature. What is the value of the reaction quotient, \\(Q_c\\), immediately after the volume expansion?"
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url: "https://nerd-notes.com/ubq/120282/"
date_modified: "2026-08-23T04:04:15+00:00"
---

# A reversible reaction is represented by the equation below.

\[ \text{N}_2\text{O}_4(g) \rightleftharpoons 2\,\text{NO}_2(g) \]

At a constant temperature, the system is initially at equilibrium in a \(1.0\text{ L}\) rigid container. At equilibrium, the concentration of \(\text{N}_2\text{O}_4(g)\) is \(0.20\text{ M}\) and the concentration of \(\text{NO}_2(g)\) is \(0.40\text{ M}\). The volume of the container is rapidly expanded to \(2.0\text{ L}\) at the same temperature. What is the value of the reaction quotient, \(Q_c\), immediately after the volume expansion?

A reversible reaction is represented by the equation below.

\[ \text{N}_2\text{O}_4(g) \rightleftharpoons 2\,\text{NO}_2(g) \]

At a constant temperature, the system is initially at equilibrium in a \(1.0\text{ L}\) rigid container. At equilibrium, the concentration of \(\text{N}_2\text{O}_4(g)\) is \(0.20\text{ M}\) and the concentration of \(\text{NO}_2(g)\) is \(0.40\text{ M}\). The volume of the container is rapidly expanded to \(2.0\text{ L}\) at the same temperature. What is the value of the reaction quotient, \(Q_c\), immediately after the volume expansion?

- **A.** \(0.20\)
- **B.** \(0.40\)
- **C.** \(0.80\)
- **D.** \(1.6\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120282/*