---
title: "The decomposition of a solid metal carbonate is represented by the following equation:  \\[ \\text{MCO}_3(s) \\rightleftharpoons \\text{MO}(s) + \\text{CO}_2(g) \\]  For this process, \\(\\Delta H^\\circ = +88\\text{ kJ/mol}_{rxn}\\) and \\(\\Delta S^\\circ = +110\\text{ J/}(\\text{mol}_{rxn}\\cdot\\text{K})\\). Assuming that \\(\\Delta H^\\circ\\) and \\(\\Delta S^\\circ\\) do not change significantly with temperature, at approximately what minimum temperature does the reaction become thermodynamically favorable under standard conditions?"
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url: "https://nerd-notes.com/ubq/119804/"
date_modified: "2026-08-21T08:12:23+00:00"
---

# The decomposition of a solid metal carbonate is represented by the following equation:

\[ \text{MCO}_3(s) \rightleftharpoons \text{MO}(s) + \text{CO}_2(g) \]

For this process, \(\Delta H^\circ = +88\text{ kJ/mol}_{rxn}\) and \(\Delta S^\circ = +110\text{ J/}(\text{mol}_{rxn}\cdot\text{K})\). Assuming that \(\Delta H^\circ\) and \(\Delta S^\circ\) do not change significantly with temperature, at approximately what minimum temperature does the reaction become thermodynamically favorable under standard conditions?

The decomposition of a solid metal carbonate is represented by the following equation:

\[ \text{MCO}_3(s) \rightleftharpoons \text{MO}(s) + \text{CO}_2(g) \]

For this process, \(\Delta H^\circ = +88\text{ kJ/mol}_{rxn}\) and \(\Delta S^\circ = +110\text{ J/}(\text{mol}_{rxn}\cdot\text{K})\). Assuming that \(\Delta H^\circ\) and \(\Delta S^\circ\) do not change significantly with temperature, at approximately what minimum temperature does the reaction become thermodynamically favorable under standard conditions?

- **A.** \(0.80\text{ K}\)
- **B.** \(800\text{ K}\)
- **C.** \(1250\text{ K}\)
- **D.** \(9680\text{ K}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119804/*