---
title: "A \\(1.0 \\text{ L}\\) rigid reaction vessel is filled with \\(1.0 \\text{ mol}\\) of \\(\\text{NOCl}(g)\\) at a fixed temperature. The reaction proceeds according to the equation below.  \\[ 2\\,\\text{NOCl}(g) \\rightleftharpoons 2\\,\\text{NO}(g) + \\text{Cl}_2(g) \\]  At this temperature, \\(K_c = 3.2 \\times 10^{-8}\\). Based on an ICE table and assuming that the change in concentration of \\(\\text{NOCl}(g)\\) is negligible, what is the equilibrium concentration of \\(\\text{Cl}_2(g)\\)?"
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url: "https://nerd-notes.com/ubq/119369/"
date_modified: "2026-08-19T12:40:03+00:00"
---

# A \(1.0 \text{ L}\) rigid reaction vessel is filled with \(1.0 \text{ mol}\) of \(\text{NOCl}(g)\) at a fixed temperature. The reaction proceeds according to the equation below.

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

At this temperature, \(K_c = 3.2 \times 10^{-8}\). Based on an ICE table and assuming that the change in concentration of \(\text{NOCl}(g)\) is negligible, what is the equilibrium concentration of \(\text{Cl}_2(g)\)?

A \(1.0 \text{ L}\) rigid reaction vessel is filled with \(1.0 \text{ mol}\) of \(\text{NOCl}(g)\) at a fixed temperature. The reaction proceeds according to the equation below.

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

At this temperature, \(K_c = 3.2 \times 10^{-8}\). Based on an ICE table and assuming that the change in concentration of \(\text{NOCl}(g)\) is negligible, what is the equilibrium concentration of \(\text{Cl}_2(g)\)?

- **A.** \(2.0 \times 10^{-3} \text{ M}\)
- **B.** \(4.0 \times 10^{-3} \text{ M}\)
- **C.** \(6.0 \times 10^{-3} \text{ M}\)
- **D.** \(8.0 \times 10^{-3} \text{ M}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119369/*