Here is the question:
If the heat of combustion of CH4 is -802 kJ/mol, use the following information (and nothing else, don't just look up data from tables) to determine the enthalpy of reaction (kJ/mol) for the partial oxidation of methane by oxygen gas to give carbon monoxide and hydrogen gas.
CH4 (g) + H2O (g) --> CO + 3 H2 (g) delta H= 206kJ
CH4 (g) + CO2 (g) --> 2 CO + 2 H2 (g) delta H= 246 kJ
What I did:
I flipped the second equation and added the two together and got:
H2O + CO --> CO2 + 1 H2 delta H= -40kJ
I know this is wrong, because I want to get methane and oxygen on the right side and carbon monoxide and hydrogen on the right side, but I don't know where to go from here. Also, oxygen gas isn't in either of these equations, so how can I form that? Any help would be greatly appreciated. (Note: This is not a graded hw problem. I have an exam coming up and this is a suggested review problem, but its aneven numbered problem so the answer is not in the back of the book. Again, thanks in advance for any help.)