---
title: "The complete combustion of methane is represented by the thermochemical equation below.  \\[ \\text{CH}_4\\text{(g)} + 2\\,\\text{O}_2\\text{(g)} \\rightarrow \\text{CO}_2\\text{(g)} + 2\\,\\text{H}_2\\text{O(l)} \\quad \\Delta H^\\circ_{\\text{rxn}} = -890\\text{ kJ/mol}_{\\text{rxn}} \\]  What is the total enthalpy change when \\(2.50\\text{ mol}\\) of \\(\\text{CH}_4\\text{(g)}\\) reacts completely with excess oxygen gas?"
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url: "https://nerd-notes.com/ubq/119676/"
date_modified: "2026-08-21T08:12:01+00:00"
---

# The complete combustion of methane is represented by the thermochemical equation below.

\[ \text{CH}_4\text{(g)} + 2\,\text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} + 2\,\text{H}_2\text{O(l)} \quad \Delta H^\circ_{\text{rxn}} = -890\text{ kJ/mol}_{\text{rxn}} \]

What is the total enthalpy change when \(2.50\text{ mol}\) of \(\text{CH}_4\text{(g)}\) reacts completely with excess oxygen gas?

The complete combustion of methane is represented by the thermochemical equation below.

\[ \text{CH}_4\text{(g)} + 2\,\text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} + 2\,\text{H}_2\text{O(l)} \quad \Delta H^\circ_{\text{rxn}} = -890\text{ kJ/mol}_{\text{rxn}} \]

What is the total enthalpy change when \(2.50\text{ mol}\) of \(\text{CH}_4\text{(g)}\) reacts completely with excess oxygen gas?

- **A.** \(-2230\text{ kJ}\)
- **B.** \(-890\text{ kJ}\)
- **C.** \(-356\text{ kJ}\)
- **D.** \(+2230\text{ kJ}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119676/*