I. AHrxn for the reaction below was determined using bond dissociation energies (BDES) to be -57 kJ. Using the table of BDE below, find the bond energy for H-Br. H H C=C H H + HBr Bond BDE (kJ/mol) H Br H-C-C-H HH C-C 348 C=C C-H 614 413 C-Br 276 II. Use heats of formation to find the standard heat of reaction (AH° rxn) for the reaction shown above. C₂H4 and HBr are both gases and AH°f for CH3CH₂Br (l) is -85.3 kJ/mol. Use T16-4-1 to find any additional values of AH°f needed. III. Why is there a dfference between the reaction enthalpies calculated by these different approaches?

I. AHrxn for the reaction below was determined using bond dissociation energies (BDES) to be -57 kJ. Using the table of BDE below, find the bond energy for H-Br. H H C=C H H + HBr Bond BDE (kJ/mol) H Br H-C-C-H HH C-C 348 C=C C-H 614 413 C-Br 276 II. Use heats of formation to find the standard heat of reaction (AH° rxn) for the reaction shown above. C₂H4 and HBr are both gases and AH°f for CH3CH₂Br (l) is -85.3 kJ/mol. Use T16-4-1 to find any additional values of AH°f needed. III. Why is there a dfference between the reaction enthalpies calculated by these different approaches?

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

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 135AE: Use bond energies (table 3-3), values of electron affinities (table 2-7), and the ionization energy...

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