I understand that the enthalpy change of formation is the formation of 1 mole of a compound from its constituent elements, with all substances in their standard states at 1 atmosphere (1 atm or 101.3 kPa).
The equation used to calculate the enthalpy of formation of water is:
H2(g)+1/2 O2(g)----------------> H2O(l)
I understand this equation as all the substances are in the standard states.
However I don't understand the equation:
H2(g)+1/2 O2(g)----------------> H2O(g)
As H2O isn't a gas in it's standard state.
Basically I don't understand how you can calculate the enthalpy change of formation for water vapour when H2O isn't a gas in it's standard state, yet the definition states that all substances must be in their standard states.
Can anyone please help me?