# Key Terms Associated with Phase Diagrams Example:
Water vapor at 1 atm and 110oC. Removing a small amount of energy would not cause any of the vapor to condense, but the temperature would decrease. Example
:
Water vapor at 1 atm and 100oC. Removing a small amount of energy would cause some of the vapor to condense into a saturated liquid, but the temperature would not change. Example
:
Water liquid and vapor in equilibrium at 1 atm and 100oC. Removing a small amount of energy would cause some of the vapor to condense, but the temperature would not decrease. Adding a small amount of energy would cause some of the liquid to vaporize, but the temperature would not increase. Example
:
Liquid water at 1 atm and 100oC. Any additional energy would cause some of the liquid to vaporize into a saturated vapor, but the temperature would not increase. Example:
Liquid water at 1 atm and 80oC. Adding a small amount of energy would not cause any of the liquid to vaporize, but the temperature would increase.
Subcooled Liquid :
Saturated Liquid :
Saturated Mixture :
Saturated Vapor :
Superheated Vapor:
A liquid at a temperature below its boiling point ( T < Tsat ) for the existing pressure.
A liquid at exactly the temperature ( Tsat ) at which it would boil at the existing pressure ( P = P* ).
A mixture of saturated liquid and saturated vapor in equilibrium. The temperature is the saturation temperature, Tsat ,and the pressure is called the vapor pressure P*= P.
A vapor at exactly the temperature ( Tsat ) at which it would condense at the existing pressure ( P = P* ).
A vapor at a temperature above its boiling point ( T > Tsat ) for the existing pressure.
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