In a molecule with multiple equivalent C-H bonds, the initial bond generally requires the highest energy to break, which is 439 kJ/mol. Subsequent bonds have an average dissociation energy of 415 kJ/mol due to alterations in the molecular structure post the first bond breaking.
The question concerns the dissociation energy required to break various C-H bonds within a molecule. While the exact bond dissociation energy of a C-H bond depends on the molecule, C-H bonds generally have similar bond energies of roughly 100 kcal/mol. However, not all C-H bonds in a molecule require the same energy to break. After breaking the first bond, subsequent bonds may require less energy to break due to changes in the molecule's structure. Specifically, the first bond requires 439 kJ/mol, and then the average energy for the remaining bonds is calculated as 415 kJ/mol, which is derived from dividing the total energy required to break all C-H bonds in the molecule (1660 kJ/mol) by four.
The complete question is- In the molecule shown below, determine which of the highlighted C-H bonds (from a to e) is expected to have the lowest bond dissociation energy .