If hydrogen were used as a fuel, it could be burned according to the following reaction:
H2(g)+1/2O2(g)→H2O(g)
Use average bond energies to calculate ΔHrxn for this reaction.
Use average bond energies to calculate ΔHrxn for the combustion of methane (CH4).
Which fuel yields more energy per mole?
Per gram?
I'd appreciate someone walking me through this more than just giving me the answer.

Question

If hydrogen were used as a fuel, it could be burned according to the following reaction: 
H2(g)+1/2O2(g)→H2O(g)
Use average bond energies to calculate ΔHrxn for this reaction.
Use average bond energies to calculate ΔHrxn for the combustion of methane (CH4).
Which fuel yields more energy per mole?
Per gram?
I'd appreciate someone walking me through this more than just giving me the answer.

sweetburger · Answer

First were going to need a list of average bond energies. Do you happen to have one?

sweetburger · Answer

http://butane.chem.uiuc.edu/cyerkes/Chem104ACSpring2009/Genchemref/bondenergies.html Here is a list in kJ/mol