First note that P2O5 is generally assumed to be in reality P4O10 (also written as (P2O5)2 or O10P4).
Note also that the mol weight of P4O10 is twice that of P2O5 so one has to be careful when using reported data per mol.
Now see the NIST-JANAF Thermochemical Table for crystal and gas P4O10 that I attached.
P4O10 thermo data from JANAF.pdf 296.27KB
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By interpolation of the data for P4O10(gas) you find that at 591 oC = 864 K the gas enthalpy (relative to gas at 298 K) is 148 kJ/mol and gas enthalpy at 60 oC = 333 K is 7 kJ/mol. See Ho - Ho(Tr) column in table.
Heat of sublimation of P4O10 at 60 oC is 104 kJ/mol (is heat of formation difference between gas and crystal at that temperature, see ΔfHo column in tables).
So total enthalpy difference between P4O10 gas at 591 oC and crystals at 60 oC is:
(148 - 7) + 104 = 245 kJ/mol P4O10 = 863 kJ/kg
In reality the transition between gas and crystal does not occur at 60 oC, but for the total enthalpy difference that does not matter. Nevertheless you can do the same exercise yourself by assuming that sublimation takes place at say 360 oC = 633 K. First use the gas table to obtain enthalpy difference between 591 and 360 oC; then determine heat of sublimation at 360 oC (from heats of formation); and then use crystal table to determine enthalpy difference between 360 to 60 oC. Add it all up and you should get practically the same value for the total enthalpy difference as I calculated before.