---
title: "A \\(1.2\\text{ mol}\\) sample of \\(\\text{NOCl(g)}\\) is placed into a previously evacuated, rigid \\(2.0\\text{ L}\\) container and heated to \\(500\\text{ K}\\). The system reaches equilibrium according to the equation below.  \\[ 2\\text{NOCl(g)} \\rightleftharpoons 2\\text{NO(g)} + \\text{Cl}_2\\text{(g)} \\]  At equilibrium, analysis shows that \\(0.40\\text{ mol}\\) of \\(\\text{Cl}_2\\text{(g)}\\) is present in the container. Based on these data, what is the value of the equilibrium constant, \\(K_c\\), for the reaction at \\(500\\text{ K}\\)?"
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/121485/"
date_modified: "2026-08-23T05:04:49+00:00"
---

# A \(1.2\text{ mol}\) sample of \(\text{NOCl(g)}\) is placed into a previously evacuated, rigid \(2.0\text{ L}\) container and heated to \(500\text{ K}\). The system reaches equilibrium according to the equation below.

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

At equilibrium, analysis shows that \(0.40\text{ mol}\) of \(\text{Cl}_2\text{(g)}\) is present in the container. Based on these data, what is the value of the equilibrium constant, \(K_c\), for the reaction at \(500\text{ K}\)?

A \(1.2\text{ mol}\) sample of \(\text{NOCl(g)}\) is placed into a previously evacuated, rigid \(2.0\text{ L}\) container and heated to \(500\text{ K}\). The system reaches equilibrium according to the equation below.

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

At equilibrium, analysis shows that \(0.40\text{ mol}\) of \(\text{Cl}_2\text{(g)}\) is present in the container. Based on these data, what is the value of the equilibrium constant, \(K_c\), for the reaction at \(500\text{ K}\)?

- **A.** \(0.050\)
- **B.** \(0.20\)
- **C.** \(0.40\)
- **D.** \(0.80\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121485/*