Calculate the enthalpy of reaction (in kJ/mol) of the combustion of ethanol USING Hess's Law?

Here is what I have...

The balanced equation I have for ethanol is: C2H5OH(l) + 3O2(g) -> 2CO2(g) + 3H2O(g)

And from that, the three equations I have are:

C + O2 -> CO2 ... deta H = -393.5

H2 + 0.5OH -> H2O ... deta H = -241. 8

2C + 3H2 + 0.5O2 -> C2H5OH ... deta H = -277.7

Then I got:

(277.7) - (2 x 393.5) - (3 x 241.

= -1234.7 kJ/mol

Is that correct? I'm not sure if the heat change's are completely right. Thank you for the help.

Edit: Also please calculate the enthalpy of reaction for one gallon of ethanol (in kJ). I am confused by this. Thank you.