Thanks for helping! THIS is the equation N2H4 + O2 → N2 + H2O First just Use bond energy values from below to Calculate the overall energy of the reaction. Then decide if the reaction is exothermic or endothermic

Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Thanks for helping!

THIS is the equation N2H4 + O2 → N2 + H2O

First just Use bond energy values from below to Calculate the overall energy of the reaction.

Then decide if the reaction is exothermic or endothermic.

 

### Average Bond Energies (kJ/mol)

Understanding bond energies is crucial for comprehending chemical reactions and properties. The following table lists the average bond energies for different chemical bonds, measured in kilojoules per mole (kJ/mol):

| Bond   | Energy (kJ/mol) | Bond   | Energy (kJ/mol) | Bond   | Energy (kJ/mol) |
|--------|------------------|--------|------------------|--------|------------------|
| H-H    | 436 kJ/mol       | C-H    | 413 kJ/mol       | C=C    | 614 kJ/mol       |
| H-Cl   | 431 kJ/mol       | C-C    | 348 kJ/mol       | C≡C    | 839 kJ/mol       |
| H-F    | 567 kJ/mol       | C-N    | 293 kJ/mol       | C=O    | 799 kJ/mol       |
| N-H    | 391 kJ/mol       | C-O    | 358 kJ/mol       | O=O    | 495 kJ/mol       |
| N-O    | 201 kJ/mol       | C-F    | 485 kJ/mol       | O=P    | 1072 kJ/mol      |
| O-H    | 463 kJ/mol       | C-Cl   | 328 kJ/mol       | C=N    | 615 kJ/mol       |
| O-O    | 146 kJ/mol       | C-S    | 259 kJ/mol       | N=N    | 418 kJ/mol       |
| F-F    | 155 kJ/mol       | Cl-Cl  | 242 kJ/mol       | N≡N    | 941 kJ/mol       |
                                                                 | C≡N    | 891 kJ/mol       |

#### Explanation of the Table:
- **Single Bonds (e.g., H-H, C-H, N-H):** These typically involve sharing one pair of electrons between atoms.
- **Double Bonds (e.g., C=C, C=O):** These involve two pairs of electrons shared between atoms, resulting in stronger bonds than single bonds.
- **Triple Bonds (e.g., C≡C, N≡N):** These bonds involve three pairs of shared electrons, contributing to even stronger bonds compared to single and double bonds.

####
Transcribed Image Text:### Average Bond Energies (kJ/mol) Understanding bond energies is crucial for comprehending chemical reactions and properties. The following table lists the average bond energies for different chemical bonds, measured in kilojoules per mole (kJ/mol): | Bond | Energy (kJ/mol) | Bond | Energy (kJ/mol) | Bond | Energy (kJ/mol) | |--------|------------------|--------|------------------|--------|------------------| | H-H | 436 kJ/mol | C-H | 413 kJ/mol | C=C | 614 kJ/mol | | H-Cl | 431 kJ/mol | C-C | 348 kJ/mol | C≡C | 839 kJ/mol | | H-F | 567 kJ/mol | C-N | 293 kJ/mol | C=O | 799 kJ/mol | | N-H | 391 kJ/mol | C-O | 358 kJ/mol | O=O | 495 kJ/mol | | N-O | 201 kJ/mol | C-F | 485 kJ/mol | O=P | 1072 kJ/mol | | O-H | 463 kJ/mol | C-Cl | 328 kJ/mol | C=N | 615 kJ/mol | | O-O | 146 kJ/mol | C-S | 259 kJ/mol | N=N | 418 kJ/mol | | F-F | 155 kJ/mol | Cl-Cl | 242 kJ/mol | N≡N | 941 kJ/mol | | C≡N | 891 kJ/mol | #### Explanation of the Table: - **Single Bonds (e.g., H-H, C-H, N-H):** These typically involve sharing one pair of electrons between atoms. - **Double Bonds (e.g., C=C, C=O):** These involve two pairs of electrons shared between atoms, resulting in stronger bonds than single bonds. - **Triple Bonds (e.g., C≡C, N≡N):** These bonds involve three pairs of shared electrons, contributing to even stronger bonds compared to single and double bonds. ####
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