I am currently reading a textbook called Engineering and Chemical Thermodynamics but I am stuck in one part about the State Postulate and the Gibbs Phase Rule. The Gibbs Phase rule says that the number of independent intensive properties that one needs to specify to constrain the properties of a given phase is:
n = Number of Chemical Species - Number of Phases + 2
Therefore, if there is a two-phase system with one chemical species, such as boiling water, one needs to specify one property in each phase to constrain all the other properties of that phase. However, the author states that we can take advantage of the fact that "the properties Temperature and Pressure are equal in both phases, thus, if we know either T or P of the system, we constrain the properties in each of the phases". This statement confused me a lot because the author didn't mention if this applies only for a saturated system. For me, it is logical that the temperature of both of the phases should be the same even if the system is not saturated, however, I am struggling to understand why the pressure of the system is the same for both phases always? The water could be boiling at 100 ºC, which means that the vapor pressure of the liquid water should be 1 atm, but the system could not be saturated and therefore the pressure of the vapor would not be 1 atm.
I assume that the author says that this applies even for unsaturated systems because of the following lines:
To illustrate this concept, consider a pure system of boiling water where we have both a liquid and a vapor phase. The phase rule tells us that for the liquid phase of water, we need only one property to constrain the state of the phase. If we know the system pressure, P, all the other properties (T, vl , ul...) of the liquid are constrained. The subscript “l” refers to the liquid phase. It is omitted on T since the temperatures of both the liquid and vapor phases are equal. For example, for a pressure of 1 atm, the temperature is 100 °C. We can also determine that the volume of the liquid is 1.04x10-3 m3/kg, the internal energy is 418.94 kJ/kg, and so on. The system pressure of 1 atm also constrains the properties of the vapor phase. The temperature remains the same as for the liquid, 100 °C; however, the values for the volume of the vapor (1.63 m3/kg), the internal energy (2,506.5 kJ/kg), and so on are different from those of the liquid.
Then he said:
The pressure (and temperature) in each phase of a two-phase system is equal; hence, if we know P (or T), we know the values of all the intensive properties in both phases. However, we have not yet constrained the state of the system. To do so, we need to know the proportion of matter in each phase. Thus, a second independent intensive property that is related to the mass fraction in each phase is required. Specifying that a system of boiling water is at 1 atm does not tell us how much liquid and how much vapor are present. We could have all liquid with just one bubble of vapor, all vapor with just one drop of liquid, or anything in between.
If my question isn't clear enough: if we have "all liquid with just one bubble of vapor", how is it possible that the pressure in each phase is equal?, this is confusing me a lot. The only explanation that I can find is that the vapor pressure of the liquid is the same as the vapor pressure of the vapor, however I don't know if the concept of vapor pressure applies for a vapor.
I would appreciate if someone can clear my doubts on this question. For more details, the chapter of the textbook is 1.5 of the 2nd edition. If I didn't explain myself enough, please let me know. Thanks in advance.