**Bond Enthalpy**Use the given bond enthalpies to estimate the ΔH for the combustion of 1 mole of methanol. **Average Bond Enthalpies:**- C–H: 413 kJ/mol- C–O: 358 kJ/mol- O–O: 146 kJ/mol- C–C: 348 kJ/mol- C=C: 614 kJ/mol- C=O: 799 kJ/mol- O–H: 463 kJ/mol- O=O: 495 kJ/mol**Chemical Reaction:**\[ \text{CH}_3\text{OH} + \frac{3}{2} \text{O}_2 \rightarrow \text{CO}_2 + 2 \text{H}_2\text{O} \]

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6. Bond enthalpy Use the given bond enthalpies to estimate the AH for the combustion of 1 mole of methanol. Average Bond Enthalpies: C- H: 413 kJ/mol C- 0: 358 kJ/mol 0-0: 146 kJ/mol C-C: 348 kJ/mol C= 0: 799 kJ/mol O = 0: 495 kJ/mol C= C: 614 kJ/mol O- H: 463 kJ/mol 3 CH3OH+02¬CO02 + 2H20

6. Bond enthalpy Use the given bond enthalpies to estimate the AH for the combustion of 1 mole of methanol. Average Bond Enthalpies: C- H: 413 kJ/mol C- 0: 358 kJ/mol 0-0: 146 kJ/mol C-C: 348 kJ/mol C= 0: 799 kJ/mol O = 0: 495 kJ/mol C= C: 614 kJ/mol O- H: 463 kJ/mol 3 CH3OH+02¬CO02 + 2H20

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

**Bond Enthalpy**

Use the given bond enthalpies to estimate the ΔH for the combustion of 1 mole of methanol.

**Average Bond Enthalpies:**

- C–H: 413 kJ/mol
- C–O: 358 kJ/mol
- O–O: 146 kJ/mol
- C–C: 348 kJ/mol
- C=C: 614 kJ/mol
- C=O: 799 kJ/mol
- O–H: 463 kJ/mol
- O=O: 495 kJ/mol

**Chemical Reaction:**

\[ \text{CH}_3\text{OH} + \frac{3}{2} \text{O}_2 \rightarrow \text{CO}_2 + 2 \text{H}_2\text{O} \]

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