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2 H₂O Bond Bond total bond energy for the reactants in the energy (kJ/mol) Average Bond Energies (per mole of bonds) H-H C-H C-C C=C 0-H bustion of ethene: 432 413 347 614 C-0 C=0 0=0 0-0 467 358 799* 495 146

2 H₂O Bond Bond total bond energy for the reactants in the energy (kJ/mol) Average Bond Energies (per mole of bonds) H-H C-H C-C C=C 0-H bustion of ethene: 432 413 347 614 C-0 C=0 0=0 0-0 467 358 799* 495 146

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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O: 0=0 0=0 O 3751 kJ/mol O O2512 kJ/mol O 1522 kJ/mol O=0. Total Energy Transferred In (positive) 0=0 0=0
Transcribed Image Text:O: 0=0 0=0 O 3751 kJ/mol O O2512 kJ/mol O 1522 kJ/mol O=0. Total Energy Transferred In (positive) 0=0 0=0
Using the table of average bond energies, determine the total bond energy for the reactants in the combustion of ethene: C₂H4 + 3 02 --> 2 CO₂ + 2 H₂O Average Bond Energies (per mole of bonds) H-H C-HCC G=6|0–H C=C C-0 Bond energy (kJ/mol) 432 413 347 614 467 Bond Molecular Structure H H C-C HH OO Bond Broken C-H C=C 0=0 Bond Energy (kJ/mol) 358 Number of Bonds Broken C=0 0-0 0-0 799* 495 Net Energy (kJ/mol) 146
Transcribed Image Text:Using the table of average bond energies, determine the total bond energy for the reactants in the combustion of ethene: C₂H4 + 3 02 --> 2 CO₂ + 2 H₂O Average Bond Energies (per mole of bonds) H-H C-HCC G=6|0–H C=C C-0 Bond energy (kJ/mol) 432 413 347 614 467 Bond Molecular Structure H H C-C HH OO Bond Broken C-H C=C 0=0 Bond Energy (kJ/mol) 358 Number of Bonds Broken C=0 0-0 0-0 799* 495 Net Energy (kJ/mol) 146
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