---
title: "A student models the complete atomization of carbon-containing gases in a high-temperature plasma reactor. The two carbon–oxygen bonds in \\(\\text{CO}_2\\text{(g)}\\) are equivalent.  | Atomization process | \\(\\Delta H\\) | |—|—:| | \\(\\text{CO(g)} \\rightarrow \\text{C(g)} + \\text{O(g)}\\) | \\(+1070\\ \\text{kJ/mol}\\) | | \\(\\text{CO}_2\\text{(g)} \\rightarrow \\text{C(g)} + 2\\text{O(g)}\\) | \\(+1600\\ \\text{kJ/mol}\\) |  Which choice correctly ranks the carbon–oxygen bond enthalpies from greatest to least and gives the best justification?"
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date_modified: "2026-08-19T12:40:18+00:00"
---

# A student models the complete atomization of carbon-containing gases in a high-temperature plasma reactor. The two carbon–oxygen bonds in \(\text{CO}_2\text{(g)}\) are equivalent.

| Atomization process | \(\Delta H\) |
|—|—:|
| \(\text{CO(g)} \rightarrow \text{C(g)} + \text{O(g)}\) | \(+1070\ \text{kJ/mol}\) |
| \(\text{CO}_2\text{(g)} \rightarrow \text{C(g)} + 2\text{O(g)}\) | \(+1600\ \text{kJ/mol}\) |

Which choice correctly ranks the carbon–oxygen bond enthalpies from greatest to least and gives the best justification?

A student models the complete atomization of carbon-containing gases in a high-temperature plasma reactor. The two carbon–oxygen bonds in \(\text{CO}_2\text{(g)}\) are equivalent.

| Atomization process | \(\Delta H\) |
|---|---:|
| \(\text{CO(g)} \rightarrow \text{C(g)} + \text{O(g)}\) | \(+1070\ \text{kJ/mol}\) |
| \(\text{CO}_2\text{(g)} \rightarrow \text{C(g)} + 2\text{O(g)}\) | \(+1600\ \text{kJ/mol}\) |

Which choice correctly ranks the carbon–oxygen bond enthalpies from greatest to least and gives the best justification?

- **A.** Bond enthalpy in \(\text{CO(g)}\) \(>\) bond enthalpy of either bond in \(\text{CO}_2\text{(g)}\), because molecules containing more atoms generally have weaker bonds.
- **B.** Bond enthalpy in \(\text{CO(g)}\) \(>\) bond enthalpy of either bond in \(\text{CO}_2\text{(g)}\), because the average bond enthalpy in \(\text{CO}_2\text{(g)}\) is \(\dfrac{1600}{2}=800\ \text{kJ/mol}\).
- **C.** Bond enthalpy of either bond in \(\text{CO}_2\text{(g)}\) \(>\) bond enthalpy in \(\text{CO(g)}\), because \(\dfrac{1600}{2}=800\ \text{kJ/mol}\), and a smaller bond enthalpy indicates a stronger bond.
- **D.** Bond enthalpy of either bond in \(\text{CO}_2\text{(g)}\) \(>\) bond enthalpy in \(\text{CO(g)}\), because \(1600\ \text{kJ/mol}>1070\ \text{kJ/mol}\).

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119429/*