---
title: "Synthesis gas, a mixture of carbon monoxide and hydrogen gas, is produced industrially by reacting solid carbon with steam according to the following equation:  \\[ \\text{C}(s) + \\text{H}_2\\text{O}(g) \\rightarrow \\text{CO}(g) + \\text{H}_2(g) \\]  The standard enthalpy changes for three related thermochemical equations are given in the table below.  | Equation | Reaction | \\(\\Delta H^\\circ\\) (\\(\\text{kJ/mol}_{rxn}\\)) | | :— | :— | :— | | (1) | \\(\\text{C}(s) + \\text{O}_2(g) \\rightarrow \\text{CO}_2(g)\\) | \\(-394\\) | | (2) | \\(2\\,\\text{CO}(g) + \\text{O}_2(g) \\rightarrow 2\\,\\text{CO}_2(g)\\) | \\(-566\\) | | (3) | \\(2\\,\\text{H}_2(g) + \\text{O}_2(g) \\rightarrow 2\\,\\text{H}_2\\text{O}(g)\\) | \\(-484\\) |  Based on the information provided, what is the value of \\(\\Delta H^\\circ\\) for the reaction \\(\\text{C}(s) + \\text{H}_2\\text{O}(g) \\rightarrow \\text{CO}(g) + \\text{H}_2(g)\\)?"
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date_modified: "2026-08-23T05:02:01+00:00"
---

# Synthesis gas, a mixture of carbon monoxide and hydrogen gas, is produced industrially by reacting solid carbon with steam according to the following equation:

\[ \text{C}(s) + \text{H}_2\text{O}(g) \rightarrow \text{CO}(g) + \text{H}_2(g) \]

The standard enthalpy changes for three related thermochemical equations are given in the table below.

| Equation | Reaction | \(\Delta H^\circ\) (\(\text{kJ/mol}_{rxn}\)) |
| :— | :— | :— |
| (1) | \(\text{C}(s) + \text{O}_2(g) \rightarrow \text{CO}_2(g)\) | \(-394\) |
| (2) | \(2\,\text{CO}(g) + \text{O}_2(g) \rightarrow 2\,\text{CO}_2(g)\) | \(-566\) |
| (3) | \(2\,\text{H}_2(g) + \text{O}_2(g) \rightarrow 2\,\text{H}_2\text{O}(g)\) | \(-484\) |

Based on the information provided, what is the value of \(\Delta H^\circ\) for the reaction \(\text{C}(s) + \text{H}_2\text{O}(g) \rightarrow \text{CO}(g) + \text{H}_2(g)\)?

Synthesis gas, a mixture of carbon monoxide and hydrogen gas, is produced industrially by reacting solid carbon with steam according to the following equation:

\[ \text{C}(s) + \text{H}_2\text{O}(g) \rightarrow \text{CO}(g) + \text{H}_2(g) \]

The standard enthalpy changes for three related thermochemical equations are given in the table below.

| Equation | Reaction | \(\Delta H^\circ\) (\(\text{kJ/mol}_{rxn}\)) |
| :--- | :--- | :--- |
| (1) | \(\text{C}(s) + \text{O}_2(g) \rightarrow \text{CO}_2(g)\) | \(-394\) |
| (2) | \(2\,\text{CO}(g) + \text{O}_2(g) \rightarrow 2\,\text{CO}_2(g)\) | \(-566\) |
| (3) | \(2\,\text{H}_2(g) + \text{O}_2(g) \rightarrow 2\,\text{H}_2\text{O}(g)\) | \(-484\) |

Based on the information provided, what is the value of \(\Delta H^\circ\) for the reaction \(\text{C}(s) + \text{H}_2\text{O}(g) \rightarrow \text{CO}(g) + \text{H}_2(g)\)?

- **A.** \(-919\text{ kJ/mol}_{rxn}\)
- **B.** \(+131\text{ kJ/mol}_{rxn}\)
- **C.** \(+373\text{ kJ/mol}_{rxn}\)
- **D.** \(+656\text{ kJ/mol}_{rxn}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121385/*