"Vapor–liquid equilibrium" is a condition in which a liquid and its vapor are in equilibrium with each other, a condition or state where the rate of evaporation equals the rate of condensation on a molecular level such that there is no net vapor–liquid interconversion. A substance at vapor–liquid equilibrium is generally referred to as a "saturated fluid". For a pure chemical substance, this implies that it is at its boiling point. The notion of "saturated fluid" includes saturated liquid , saturated liquid–vapor mixture, and saturated vapor .
Although theoretically equilibrium is never reached, equilibrium is practically reached in a relatively closed location if a liquid and its vapor are allowed to stand in contact with each other with no interference or only gradual interference from the outside. However, this does not apply to cases of intensive heat exchange or rapid pressure change.
The concentration of a vapor in contact with its liquid, especially at equilibrium, is often expressed in terms of vapor pressure, which will be a partial pressure if any other gas are present with the vapor. The equilibrium vapor pressure of a liquid is in general strongly dependent on temperature. At vapor–liquid equilibrium, a liquid with individual components in certain concentrations will have an equilibrium vapor in which the concentrations or partial pressures of the vapor components have certain values depending on all of the liquid component concentrations and the temperature. The converse is also true: if a vapor with components at certain concentrations or partial pressures is in vapor–liquid equilibrium with its liquid, then the component concentrations in the liquid will be determined dependent on the vapor concentrations and on the temperature. The equilibrium concentration of each component in the liquid phase is often different from its concentration in the vapor phase, but there is a relationship. The VLE concentration data can be determined experimentally, or computed or approximated with the help of theories such as Raoult's law, Dalton's law, and Henry's law.
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