Why there is a change in enthalpy in phase transition?

I'm asking because enthalpy depends only on temperature:

$$\mathrm dH = C_p\,\mathrm dT,$$

and the change in temperature is $\mathrm dT = 0.$

  • 2
    $\begingroup$ It depends on n, P, V. too. dH = Q isn't general as in your statement. Your book or notes should have all. $\endgroup$ – Alchimista Jul 16 '19 at 10:14

For a single phase, enthalpy is a function of temperature and pressure, and, at constant pressure, $\mathrm dH = C_p\,\mathrm dT.$

However, at a change of phase, enthalpy (per unit mass) undergoes a jump change, even at constant temperature and pressure. If the phase change is from liquid to vapor, for example, this jump change in enthalpy is called the heat of vaporization.


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