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12.1: Phase Stability
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We have already encountered the gas, liquid, and solid phases and already discussed some of their properties. These terms are intuitive since these are the three most common states of matter.
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12.2: Gibbs Phase Rule
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In chapter 1, we have already seen that the number of independent variables required to describe an ideal gas is two. This number was derived by counting the total number of variables (3:P,V¯,T), and reduce it by one because the ideal gas law constrains the value of one of them, once the other two are fixed.
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12.3: PT Phase Diagrams
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Let’s now discuss the pressure–temperature diagram of a typical substance, as reported in Figure 12.3.1. Each of the lines reported in the diagram represents an equilibrium between two phases, and therefore it represents a condition that reduces the number of degrees of freedom to one.
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12.4: The Clausius-Clapeyron Equation
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Let’s now take a closer look at the equilibrium between a condensed phase and the gas phase.