---
title: "The following reactions and their equilibrium constants at \\(1000\\text{ K}\\) are given:  \\[\\text{CO}(g) + \\frac{1}{2}\\,\\text{O}_2(g) \\rightleftharpoons \\text{CO}_2(g) \\quad K_1 = 1.2 \\times 10^5\\]  \\[\\text{C}(s) + \\text{CO}_2(g) \\rightleftharpoons 2\\,\\text{CO}(g) \\quad K_2 = 2.5 \\times 10^{-3}\\]  Based on these data, what is the value of the equilibrium constant, \\(K\\), for the reaction \\(\\text{C}(s) + \\text{O}_2(g) \\rightleftharpoons \\text{CO}_2(g)\\) at \\(1000\\text{ K}\\)?"
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url: "https://nerd-notes.com/ubq/119824/"
date_modified: "2026-08-21T08:12:31+00:00"
---

# The following reactions and their equilibrium constants at \(1000\text{ K}\) are given:

\[\text{CO}(g) + \frac{1}{2}\,\text{O}_2(g) \rightleftharpoons \text{CO}_2(g) \quad K_1 = 1.2 \times 10^5\]

\[\text{C}(s) + \text{CO}_2(g) \rightleftharpoons 2\,\text{CO}(g) \quad K_2 = 2.5 \times 10^{-3}\]

Based on these data, what is the value of the equilibrium constant, \(K\), for the reaction \(\text{C}(s) + \text{O}_2(g) \rightleftharpoons \text{CO}_2(g)\) at \(1000\text{ K}\)?

The following reactions and their equilibrium constants at \(1000\text{ K}\) are given:

\[\text{CO}(g) + \frac{1}{2}\,\text{O}_2(g) \rightleftharpoons \text{CO}_2(g) \quad K_1 = 1.2 \times 10^5\]

\[\text{C}(s) + \text{CO}_2(g) \rightleftharpoons 2\,\text{CO}(g) \quad K_2 = 2.5 \times 10^{-3}\]

Based on these data, what is the value of the equilibrium constant, \(K\), for the reaction \(\text{C}(s) + \text{O}_2(g) \rightleftharpoons \text{CO}_2(g)\) at \(1000\text{ K}\)?

- **A.** \(1.7 \times 10^{-13}\)
- **B.** \(2.1 \times 10^{-8}\)
- **C.** \(3.0 \times 10^2\)
- **D.** \(3.6 \times 10^7\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119824/*