---
title: "The combustion of ethane gas is represented by the following equation.  \\[\\text{C}_2\\text{H}_6(g) + \\dfrac{7}{2}\\text{O}_2(g) \\rightarrow 2\\text{CO}_2(g) + 3\\text{H}_2\\text{O}(g)\\]  | Bond | Average bond enthalpy (\\(\\text{kJ/mol}\\)) | | :— | :— | | \\(\\text{C}-\\text{C}\\) | \\(350\\) | | \\(\\text{C}-\\text{H}\\) | \\(410\\) | | \\(\\text{O}=\\text{O}\\) | \\(500\\) | | \\(\\text{C}=\\text{O}\\) | \\(800\\) | | \\(\\text{O}-\\text{H}\\) | \\(460\\) |  Based on the bond enthalpy data in the table, what is the estimated standard enthalpy of combustion, \\(\\Delta H_{\\text{comb}}^\\circ\\), for \\(1\\text{ mol}\\) of \\(\\text{C}_2\\text{H}_6(g)\\)?"
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url: "https://nerd-notes.com/ubq/119996/"
date_modified: "2026-08-21T08:31:42+00:00"
---

# The combustion of ethane gas is represented by the following equation.

\[\text{C}_2\text{H}_6(g) + \dfrac{7}{2}\text{O}_2(g) \rightarrow 2\text{CO}_2(g) + 3\text{H}_2\text{O}(g)\]

| Bond | Average bond enthalpy (\(\text{kJ/mol}\)) |
| :— | :— |
| \(\text{C}-\text{C}\) | \(350\) |
| \(\text{C}-\text{H}\) | \(410\) |
| \(\text{O}=\text{O}\) | \(500\) |
| \(\text{C}=\text{O}\) | \(800\) |
| \(\text{O}-\text{H}\) | \(460\) |

Based on the bond enthalpy data in the table, what is the estimated standard enthalpy of combustion, \(\Delta H_{\text{comb}}^\circ\), for \(1\text{ mol}\) of \(\text{C}_2\text{H}_6(g)\)?

The combustion of ethane gas is represented by the following equation.

\[\text{C}_2\text{H}_6(g) + \dfrac{7}{2}\text{O}_2(g) \rightarrow 2\text{CO}_2(g) + 3\text{H}_2\text{O}(g)\]

| Bond | Average bond enthalpy (\(\text{kJ/mol}\)) |
| :--- | :--- |
| \(\text{C}-\text{C}\) | \(350\) |
| \(\text{C}-\text{H}\) | \(410\) |
| \(\text{O}=\text{O}\) | \(500\) |
| \(\text{C}=\text{O}\) | \(800\) |
| \(\text{O}-\text{H}\) | \(460\) |

Based on the bond enthalpy data in the table, what is the estimated standard enthalpy of combustion, \(\Delta H_{\text{comb}}^\circ\), for \(1\text{ mol}\) of \(\text{C}_2\text{H}_6(g)\)?

- **A.** \(-2800\text{ kJ/mol}\)
- **B.** \(-1400\text{ kJ/mol}\)
- **C.** \(+1400\text{ kJ/mol}\)
- **D.** \(+2800\text{ kJ/mol}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119996/*