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Posted: Tue Jan 16, 2018 5:45 pm
by Natalie LeRaybaud 1G
Can someone please explain how to go about doing this problem?

Benzene is more stable and less reactive than would be predicted from its Kekulé structures. Use the mean bond enthalpies in Table 8.7 to calculate the lowering in molar energy when resonance is allowed between the Kekulé structures of benzene.

Re: 8.77

Posted: Tue Jan 16, 2018 7:56 pm
by ConnorThomas2E
In order to do this problem, you would first calculate the energies to break the bonds of 3 double bonded carbons and 3 single bonded carbons. You would then compare this value to 6 resonance carbon bonds, and see that the resonance structure requires more energy to break the bonds, and it is therefore more stable.

Re: 8.77

Posted: Tue Jan 16, 2018 10:08 pm
by Ramya Lakkaraju 1B
In the table of enthalpies, there is a specific number for the bonds found in a benzene ring.