---
title: "At \\(373\\text{ K}\\), the formation of phosgene from carbon monoxide and chlorine gas is represented by the following chemical equation.  \\[\\text{CO}(g) + \\text{Cl}_2(g) \\rightleftharpoons \\text{COCl}_2(g) \\quad K_c = 4.0 \\times 10^2\\]  What is the value of the equilibrium constant, \\(K_c’\\), for the decomposition reaction represented below at \\(373\\text{ K}\\)?  \\[\\text{COCl}_2(g) \\rightleftharpoons \\text{CO}(g) + \\text{Cl}_2(g)\\]"
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date_modified: "2026-08-21T08:31:39+00:00"
---

# At \(373\text{ K}\), the formation of phosgene from carbon monoxide and chlorine gas is represented by the following chemical equation.

\[\text{CO}(g) + \text{Cl}_2(g) \rightleftharpoons \text{COCl}_2(g) \quad K_c = 4.0 \times 10^2\]

What is the value of the equilibrium constant, \(K_c’\), for the decomposition reaction represented below at \(373\text{ K}\)?

\[\text{COCl}_2(g) \rightleftharpoons \text{CO}(g) + \text{Cl}_2(g)\]

At \(373\text{ K}\), the formation of phosgene from carbon monoxide and chlorine gas is represented by the following chemical equation.

\[\text{CO}(g) + \text{Cl}_2(g) \rightleftharpoons \text{COCl}_2(g) \quad K_c = 4.0 \times 10^2\]

What is the value of the equilibrium constant, \(K_c'\), for the decomposition reaction represented below at \(373\text{ K}\)?

\[\text{COCl}_2(g) \rightleftharpoons \text{CO}(g) + \text{Cl}_2(g)\]

- **A.** \(2.5 \times 10^{-4}\)
- **B.** \(2.5 \times 10^{-3}\)
- **C.** \(4.0 \times 10^{-2}\)
- **D.** \(4.0 \times 10^2\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119990/*