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Introduction of Phase Equilibria

Left to equilibration, several compositions will form a uniform single phase but depending on the pressure and temperature even a single substance may be separate into two or more different phases. In each phase, properties are identical but between the two phases properties are different from each other.

In a closed jar with an air space over it water forms a two phase system. Mainly the water is in liquid phase, where it is held by mutual attraction of water molecules. Molecules are constantly in motion and once in a while even at the equilibrium, in the liquid phase the molecule gains sufficient kinetic energy to break away from the liquid phase and enter in to the gas phase. Likewise, a vapor molecule collides with the liquid surface and condenses into the liquid, every once in a while. At equilibrium, evaporation and condensation processes exactly balance and there is no net change in the volume of either phase.

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At room pressure and temperature, water jar get to the equilibrium when the air over the water has a humidity of about 3%. This percentage gets increased when temperature goes up. At the 100 °C and atmospheric pressure, equilibrium is not reached until, air is 100% water. If the liquid is heated a little over 100 °C, transition from liquid to gas will occur not only at the surface but throughout the liquid volume: the water boils.

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