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title: "A sample of \\(\\text{NOCl(g)}\\) is placed into a rigid, evacuated \\(2.0\\text{ L}\\) container and heated until equilibrium is reached at \\(350^\\circ\\text{C}\\) according to the following equation:  \\[ 2\\text{NOCl(g)} \\rightleftharpoons 2\\text{NO(g)} + \\text{Cl}_2\\text{(g)} \\]  At equilibrium, the mixture contains \\(0.40\\text{ mol}\\) of \\(\\text{NOCl(g)}\\), \\(0.10\\text{ mol}\\) of \\(\\text{NO(g)}\\), and \\(0.080\\text{ mol}\\) of \\(\\text{Cl}_2\\text{(g)}\\). What is the value of the equilibrium constant, \\(K_c\\), for the reaction at this temperature?"
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url: "https://nerd-notes.com/ubq/121407/"
date_modified: "2026-08-23T05:02:07+00:00"
---

# A sample of \(\text{NOCl(g)}\) is placed into a rigid, evacuated \(2.0\text{ L}\) container and heated until equilibrium is reached at \(350^\circ\text{C}\) according to the following equation:

\[ 2\text{NOCl(g)} \rightleftharpoons 2\text{NO(g)} + \text{Cl}_2\text{(g)} \]

At equilibrium, the mixture contains \(0.40\text{ mol}\) of \(\text{NOCl(g)}\), \(0.10\text{ mol}\) of \(\text{NO(g)}\), and \(0.080\text{ mol}\) of \(\text{Cl}_2\text{(g)}\). What is the value of the equilibrium constant, \(K_c\), for the reaction at this temperature?

A sample of \(\text{NOCl(g)}\) is placed into a rigid, evacuated \(2.0\text{ L}\) container and heated until equilibrium is reached at \(350^\circ\text{C}\) according to the following equation:

\[ 2\text{NOCl(g)} \rightleftharpoons 2\text{NO(g)} + \text{Cl}_2\text{(g)} \]

At equilibrium, the mixture contains \(0.40\text{ mol}\) of \(\text{NOCl(g)}\), \(0.10\text{ mol}\) of \(\text{NO(g)}\), and \(0.080\text{ mol}\) of \(\text{Cl}_2\text{(g)}\). What is the value of the equilibrium constant, \(K_c\), for the reaction at this temperature?

- **A.** \(2.5 \times 10^{-3}\)
- **B.** \(5.0 \times 10^{-3}\)
- **C.** \(1.0 \times 10^{-2}\)
- **D.** \(5.0 \times 10^{-2}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121407/*