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title: "In industrial iron smelting, solid iron(III) oxide is reduced to iron. The thermodynamically unfavorable decomposition of \\(\\text{Fe}_2\\text{O}_3\\text{(s)}\\) is coupled with the oxidation of carbon monoxide gas, as represented by the following thermochemical equations at \\(298 \\text{ K}\\):  \\[\\text{Fe}_2\\text{O}_3\\text{(s)} \\rightarrow 2\\text{ Fe(s)} + \\dfrac{3}{2}\\text{ O}_2\\text{(g)} \\quad \\Delta G^\\circ_{298} = +740\\text{ kJ/mol}_{rxn}\\]  \\[\\text{CO(g)} + \\dfrac{1}{2}\\text{ O}_2\\text{(g)} \\rightarrow \\text{CO}_2\\text{(g)} \\quad \\Delta G^\\circ_{298} = -260\\text{ kJ/mol}_{rxn}\\]  Based on the information above, what is the value of \\(\\Delta G^\\circ_{298}\\) for the overall coupled reaction represented below?  \\[\\text{Fe}_2\\text{O}_3\\text{(s)} + 3\\text{ CO(g)} \\rightarrow 2\\text{ Fe(s)} + 3\\text{ CO}_2\\text{(g)}\\]"
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date_modified: "2026-08-23T04:23:14+00:00"
---

# In industrial iron smelting, solid iron(III) oxide is reduced to iron. The thermodynamically unfavorable decomposition of \(\text{Fe}_2\text{O}_3\text{(s)}\) is coupled with the oxidation of carbon monoxide gas, as represented by the following thermochemical equations at \(298 \text{ K}\):

\[\text{Fe}_2\text{O}_3\text{(s)} \rightarrow 2\text{ Fe(s)} + \dfrac{3}{2}\text{ O}_2\text{(g)} \quad \Delta G^\circ_{298} = +740\text{ kJ/mol}_{rxn}\]

\[\text{CO(g)} + \dfrac{1}{2}\text{ O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} \quad \Delta G^\circ_{298} = -260\text{ kJ/mol}_{rxn}\]

Based on the information above, what is the value of \(\Delta G^\circ_{298}\) for the overall coupled reaction represented below?

\[\text{Fe}_2\text{O}_3\text{(s)} + 3\text{ CO(g)} \rightarrow 2\text{ Fe(s)} + 3\text{ CO}_2\text{(g)}\]

In industrial iron smelting, solid iron(III) oxide is reduced to iron. The thermodynamically unfavorable decomposition of \(\text{Fe}_2\text{O}_3\text{(s)}\) is coupled with the oxidation of carbon monoxide gas, as represented by the following thermochemical equations at \(298 \text{ K}\):

\[\text{Fe}_2\text{O}_3\text{(s)} \rightarrow 2\text{ Fe(s)} + \dfrac{3}{2}\text{ O}_2\text{(g)} \quad \Delta G^\circ_{298} = +740\text{ kJ/mol}_{rxn}\]

\[\text{CO(g)} + \dfrac{1}{2}\text{ O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} \quad \Delta G^\circ_{298} = -260\text{ kJ/mol}_{rxn}\]

Based on the information above, what is the value of \(\Delta G^\circ_{298}\) for the overall coupled reaction represented below?

\[\text{Fe}_2\text{O}_3\text{(s)} + 3\text{ CO(g)} \rightarrow 2\text{ Fe(s)} + 3\text{ CO}_2\text{(g)}\]

- **A.** \(-1520\text{ kJ/mol}_{rxn}\)
- **B.** \(-780\text{ kJ/mol}_{rxn}\)
- **C.** \(-40\text{ kJ/mol}_{rxn}\)
- **D.** \(+480\text{ kJ/mol}_{rxn}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120344/*