One area often encountered in thermodynamics is the description of the equilibrium state of a system. We can describe a system as being in a reproducible equilibrium state when we can fix as constant some number of intensive variables. As a simple example, if an evacuated container is filled to half its volume with pure water, we would expect the system to reach equilibrium when the temperature, T, becomes constant and uniform throughout the container. Our common sense tells us that only this one intensive variable must be uniform throughout the system for the system to be at equilibrium. The Phase Rule
F = C - p + 2
where C is the number of components and p is the number of phases in the system. For our simple example above, there is one component and two phases, liquid water and water vapor, so the number of degrees of freedom is:
F = 1 - 2 + 2 = 1
The number of components can sometimes be tricky to determine. If there is a fixed relationship between chemical species, they are not separate components. For example, if sodium chloride is added to water you would not count Na+ and Cl- as separate components. Since [Na+] equals [Cl-], there is only one additional component, salt.
F = 2 - 2 + 2 = 2