The enthalpy change for each of the following reactions was calculated using bond energies. The bond energies of X–O, Y–O, and Z–O are all equal.
X–X + O=O → X–O–O–X; ∆H = –275 kJ
Y–Y + O=O → Y–O–O–Y; ∆H = +275 kJ
Z–Z + O=O → Z–O–O–Z; ∆H = –100 kJ
a. Rank the bonds X–X,Y–Y, and Z–Z from strongest to weakest.
b. Compare the energies required to completely dissociate each of the products to atoms.
c. If O2 molecules were O–O instead of O=O, how would this change ∆H for each reaction?