Raoult's law

Raoult's law states that each component's partial vapor pressure in an ideal solution equals its pure-component vapor pressure multiplied by its liquid-phase mole fraction.

Dalton's law of partial pressures: A gas mixture's total pressure equals the sum of the partial pressures of its components. It combines the component vapor pressures predicted by Raoult's law into a total pressure.
Vapor–liquid equilibrium: The condition in which vapor and liquid phases coexist without net transfer of matter between them. Raoult's law relates the liquid composition to vapor pressure at this equilibrium.
Vapor–liquid equilibrium data: Measured or modeled relationships among temperature, pressure, and liquid and vapor compositions in equilibrium. Raoult's law provides a simple baseline for estimating these relationships.
Henry's law: A relation stating that a dilute solute's partial pressure is proportional to its liquid-phase mole fraction. It describes dilute-solute behavior where Raoult's law generally does not.
François-Marie Raoult: A French chemist whose measurements of solution vapor pressures led to Raoult's law. His experimental work established the relation's empirical basis.
Vapor pressure: The pressure exerted by a vapor in equilibrium with its condensed phase at a given temperature. Raoult's law describes how solution composition changes this equilibrium pressure.
Saturation vapor pressure: The equilibrium pressure of a pure substance's vapor above its liquid or solid at a given temperature. It supplies the pure-component pressure multiplied by the solution's mole fraction.
Flash evaporation: A separation process in which part of a liquid mixture vaporizes after a sudden pressure or temperature change. Raoult-based equilibrium calculations estimate how much feed vaporizes and its composition.
Positive deviation from Raoult's law: A solution behavior in which component vapor pressures exceed the values predicted by Raoult's law. Weaker-than-ideal interactions cause the law to underpredict vapor pressures.
Colligative properties: Solution properties that depend chiefly on the number of dissolved particles rather than their chemical identity. Raoult's vapor-pressure lowering helped establish this class of solution behavior.

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