The compound oxygen difluoride is quite reactive, giving oxygen and HF when treated with water:
OF2(g) + H2O(g) --> O2(g) + 2 HF (g) ΔH°rxn = -318 kj/mole
Using bond energies, calculate the bond dissociation energy of the O-F bond in OF2(g).
According to someone on Yahoo Answers, this is how to solve it: -318 kJ/mol = BDE for OF2 + BDE for H2O - BDE for O2 - 2 x BDE for HF.
But the Bond Diassociation Energy (BDE) chart in my book has a blank space for O-F. So then how do I solve this, there must be a different method.
The answer to this question is -126kj.
Show me how to solve this..