Does the enthalpy of formation include translational and rotational energy? I can look up the enthalpy of formation of water vapor and get -241,826 KJ/mol. I want to use this to compute the total energy of water vapor at STP from the energies of O2 and H2 gas. What I don't know is whether I should use the electronic energies of H2 gas and O2 gas or the total energies of H2 gas and O2 gas, which include the contributions from the translational and rotational partition functions.
Basically, which of these two is the correct usage of Enthalpy of Formation?

ETotal(H2O) = Eelectronic(O2) + Eelectronic(H2) -241,826 KJ/mol + ETranslational(H2O) + ERotational(H2O)
ETotal(H2O) = ETotal(O2) + ETotal(H2) -241,826 KJ/mol
To add to @Kexanone's answer above, the enthalpy of formation refers to how much heat is evolved or adsorbed from the environment in a reaction. So it's the total energy, and in an ideal gas it has the form: dft + translational + rotational + vibrational + PdV, where the PdV refers to the energy needed to make space for the gas (grand canonical ensemble; in the canonical ensemble (fixed volume) this does not show up). At room temperature the vibrational and PdV terms are typically small compared to DFT energy errors (order 1 millihartree), with the PdV term only coming into play at pressures within an order of magnitude or two of those found in the detonation of thermonuclear bombs.