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DESCRIPTION: Phase diagrams are designed to depict that changes in the properties of a solution in relation to a number of variables, including temperature and pressure. There are a number of characteristics associated with these phase diagrams including: The line between phases is representative of an equilibrium. For example, point B in Figure 1 represents the boiling point, the temperature at which a substance goes from liquid to gas.
The intersection of the three lines is the triple point. This refers to the point at which the three phases exist in thermodynamic equilibrium. The endpoint of a phase diagram is known as the critical point. This refers to the point where we have a supercritical fluid. Below are the phase diagrams for two substances- H2O and CO2.
Note: These phase diagrams are only applicable for pure substances.
 Figure 1. Phase diagram for H2O (a) and CO2 (b). These figures are not drawn to scale. A/X= Triple Point, B= Melting Point, C= Boiling Point, D/Z= Critical...

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