Thermodynamic state having 2 degrees of freedom (i.e., for properties)

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SUMMARY

The discussion focuses on the thermodynamic state characterized by two degrees of freedom (DOF) and its relationship with five fundamental properties: Pressure (P), Volume (V), Temperature (T), Entropy (S), and Internal Energy (U). It establishes that with five properties, having two DOF necessitates three constraint equations, with the First Law of Thermodynamics and the Ideal Gas Law providing two of these equations. The conversation also references Gibbs' Phase Rule to explore the implications of phases and DOF in thermodynamic systems, particularly highlighting the behavior of true-extensive properties in relation to phases and saturation states.

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swampwiz
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TL;DR
What is the underlying reason that thermodynamic state has 2 degrees of freedom - i.e., that any 2 properties (saturated state excepted) completely determines the state?
I'm trying to delve into the reason why this is so. It seems that there are 5 fundamental properties:

P - Pressure
V - Volume (specific)
T - Temperature
S - Entropy (specific)
U - Internal Energy

(Yes, there are other types of energy, but they are fully determinable from these 5 - e.g., Enthalpy: H = U + PV)

Since there are 5 such possible domain variables, having a net of 2 DOF means that there must be 3 constraint equations. The 1st Law of Thermodynamics provides 1 of the equations:

dU = δQ - δW = T dS - P dV

so what are the other 2?

I can see for an ideal gas that the Ideal Gas law provides another:

p V = R T

but even for this model, there must be yet another.
 
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Do you know about "Gibbs' Phase Rule"? That might help to answer your question
 
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Master1022 said:
Do you know about "Gibbs' Phase Rule"? That might help to answer your question
So it seems that because the the 1st Law of Thermodynamics involves only 2 true-extensive properties T & P (i.e., specific Volume or Entropy is not a true-extensive property), the topology is as per a 2-D domain, with the result that phases are regions within that domain, and thus a maximum of 3 phases can exist at single points, with there being 0 DOF of those true-extensive properties there (e.g., the triple point has no DOF - it is a singular point), and such that along points at which there are 2 phases (i.e., saturation paths), there is 1 DOF of true-extensive properties (e.g., saturated water liquid/vapor has a specific temperature for a given pressure and vice-versa), and thus 2 DOF when inside a solitary phase.

However, this idea can be simplified such that the number of true-extensive properties is the number of DOF outside of a saturation state. But this doesn't explain why intensive properties are not part of the DOF. I think there is a deeper reason here.
 

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