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Distillation separates mixture components by selective boiling and condensation of vapors based on differences in relative volatility.
Distillation (also called classical distillation) is the process of separating the component substances of a liquid mixture of two or more chemically distinct substances by selectively boiling the mixture and then condensing the resulting vapors in a still. The separation works because components have different relative volatilities, so the vapor phase becomes enriched in more volatile components while the remaining liquid (the bottoms) becomes enriched in less volatile components. The purpose of distillation is to obtain high-purity separated chemicals in a convenient, time-tested way, and it can be run across a wide range of pressures and feed compositions. In industrial settings, distillation is typically treated as a physical unit operation (not a chemical reaction), and it is used for applications such as producing alcoholic beverages, desalination, crude oil stabilization, refining fuels and chemical feedstocks, and cryogenic air separation into oxygen, nitrogen, and argon.
Distillation separates mixture components by selective boiling and condensation of vapors based on differences in relative volatility.
It is used to produce high-purity products and is widely applied as a physical separation unit operation in laboratory, industrial, and food/perfumery contexts.
A separation process that boils a liquid mixture and condenses the vapors to separate its components based on volatility differences.
Heating a mixture so that components with higher volatility preferentially enter the vapor phase.
Cooling the vapor in a condenser so it returns to the liquid phase as distillate.
A measure of how readily one component vaporizes compared with another, determining how effectively they separate during distillation.
The apparatus in which the mixture is boiled and the vapor is condensed and collected as distillate.
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