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title: "A student introduces \\(\\text{N}_2\\text{O}_4\\text{(g)}\\) and \\(\\text{NO}_2\\text{(g)}\\) into a rigid, evacuated \\(1.0 \\text{ L}\\) container at \\(298 \\text{ K}\\). The reaction and its equilibrium constant at \\(298 \\text{ K}\\) are represented below.  \\[\\text{N}_2\\text{O}_4\\text{(g)} \\rightleftharpoons 2\\text{ NO}_2\\text{(g)} \\quad K_c = 4.0 \\times 10^{-2}\\]  The initial concentration of \\(\\text{N}_2\\text{O}_4\\text{(g)}\\) is \\(0.10 \\text{ M}\\) and the initial concentration of \\(\\text{NO}_2\\text{(g)}\\) is \\(0.20 \\text{ M}\\). Which of the following best predicts the direction in which the reaction will proceed to reach equilibrium, and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/119346/"
date_modified: "2026-08-19T12:39:53+00:00"
---

# A student introduces \(\text{N}_2\text{O}_4\text{(g)}\) and \(\text{NO}_2\text{(g)}\) into a rigid, evacuated \(1.0 \text{ L}\) container at \(298 \text{ K}\). The reaction and its equilibrium constant at \(298 \text{ K}\) are represented below.

\[\text{N}_2\text{O}_4\text{(g)} \rightleftharpoons 2\text{ NO}_2\text{(g)} \quad K_c = 4.0 \times 10^{-2}\]

The initial concentration of \(\text{N}_2\text{O}_4\text{(g)}\) is \(0.10 \text{ M}\) and the initial concentration of \(\text{NO}_2\text{(g)}\) is \(0.20 \text{ M}\). Which of the following best predicts the direction in which the reaction will proceed to reach equilibrium, and provides the correct justification?

A student introduces \(\text{N}_2\text{O}_4\text{(g)}\) and \(\text{NO}_2\text{(g)}\) into a rigid, evacuated \(1.0 \text{ L}\) container at \(298 \text{ K}\). The reaction and its equilibrium constant at \(298 \text{ K}\) are represented below.

\[\text{N}_2\text{O}_4\text{(g)} \rightleftharpoons 2\text{ NO}_2\text{(g)} \quad K_c = 4.0 \times 10^{-2}\]

The initial concentration of \(\text{N}_2\text{O}_4\text{(g)}\) is \(0.10 \text{ M}\) and the initial concentration of \(\text{NO}_2\text{(g)}\) is \(0.20 \text{ M}\). Which of the following best predicts the direction in which the reaction will proceed to reach equilibrium, and provides the correct justification?

- **A.** The reaction will proceed to the left because \(Q_c = 0.40\), which is greater than \(K_c\).
- **B.** The reaction will proceed to the right because \(Q_c = 0.40\), which is greater than \(K_c\).
- **C.** The reaction will proceed to the right because \(Q_c = 0.020\), which is less than \(K_c\).
- **D.** The reaction will proceed to the left because \(Q_c = 0.020\), which is less than \(K_c\).

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119346/*