Stuck on Question 8.67 [ENDORSED]

[Chiao-Wei Cheng 3e]

The question is Use the information in Tables 8.3, 8.6, and 8.7 to estimate the enthalpy of formation of each of the following compounds in
the liquid state. The standard enthalpy of sublimation of carbon is -717 kJ/mol.
(a) H 2 O; (b) methanol, CH 3 OH; (c) benzene,C 6 H 6 (without resonance); (d) benzene, C 6 H 6 (with resonance).
I have no idea how to start this problem.
For (a), do I first write out an equation for the formation of H2O, add the bond enthalpies of H-H and half of O-O and subtract the 2 bond enthalpies of the O-H bond? What else would I need to do?

[Tiffany_Luu_1F]

Yes, that is what I did but then I also had to subtract by the heat of vaporization of H2O because it is asking for the liquid state. So once you do the [bonds broken] - [bonds formed] you get -242 kj/mol, and then you subtract this by 40.7 to get -282.7 kj/mol