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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

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
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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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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