Use the data in Thermodynamic Properties and the bond energy in Bond Energies to determine the average C-C bond energy in benzene (C6H6). kJ/mol 4.0✔ Calculate the average of a C-C single bond and a C=C double bond using the bond energies, which is the value expected from the Lewis structure. kJ/mol The larger calculated value using thermodynamic properties is due to the fact that the pi system is delocalized, which makes the molecule more stable than predicted by simply averaging the C-C bonds.

Use the data in Thermodynamic Properties and the bond energy in Bond Energies to determine the average C-C bond energy in benzene (C6H6). kJ/mol 4.0✔ Calculate the average of a C-C single bond and a C=C double bond using the bond energies, which is the value expected from the Lewis structure. kJ/mol The larger calculated value using thermodynamic properties is due to the fact that the pi system is delocalized, which makes the molecule more stable than predicted by simply averaging the C-C bonds.

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

Chapter22: Organic And Biological Molecules

Section: Chapter Questions

Problem 158CP: Estimate H for the following reactions using bond energies given in Table 8.5. 3CH2=CH2(g) + 3H2(g) ...

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