00:01
Let's first calculate the delta h of formation using bond energies and see how close it is to the actual delta h of formation of benzene.
00:11
To do this, when forming benzene, we need 6 moles of gaseous carbon, so it'll be 6 times the value in table 18 .3, plus 6 moles of hydrogen, so it'll be 6 times the value in table 18 .3.
00:29
Will then subtract off.
00:32
When we form benzene, there'll be six ch bonds.
00:36
There'll be a hydrogen coming off of each of these points, each point being a carbon.
00:42
This is the bond energy for ch, according to table 18 .4.
00:48
And then three times, there's one, two, three cc bonds that are single bonds, and one, two, three, c, c, double bonds...