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.
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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