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Raoult’s Law for Ideal Solutions

1887
  • François-Marie Raoult
19th-century laboratory experiment illustrating Raoult's Law in physical chemistry.

(generated image for illustration only)

Raoult’s law states that the partial vapor pressure of each component in an ideal mixture of liquids is equal to the vapor pressure of the pure component multiplied by its mole fraction in the liquid mixture. The governing formula is \(P_i = P_i^* x_i\), where \(P_i\) is the component’s partial pressure, \(P_i^*\) is its pure vapor pressure, and \(x_i\) is its mole fraction.

Raoult’s law is a fundamental principle in physical chemistry that describes the vapor pressure of an ideal solution. An ideal solution is one where the intermolecular forces between different chemical species are the same as those between identical species. The law is expressed mathematically as \(P_i = P_i^* x_i\). Here, \(P_i\) represents the partial vapor pressure of component ‘i’ above the solution, \(P_i^*\) is the vapor pressure of the pure component ‘i’ at the same temperature, and \(x_i\) is the mole fraction of component ‘i’ in the liquid phase.

This relationship implies that dissolving a non-volatile solute (\(P_{solute}^* = 0\)) in a solvent will lower the solvent’s vapor pressure because its mole fraction \(x_{solvent}\) becomes less than 1. For a solution with multiple volatile components, the total vapor pressure above the solution can be calculated by summing the partial pressures of each component, according to Dalton’s Law of Partial Pressures: \(P_{total} = \sum_i P_i = \sum_i P_i^* x_i\). This principle is the theoretical basis for fractional distillation, a process that separates liquids with different boiling points. The component with the higher pure vapor pressure (\(P_i^*\)) will be more concentrated in the vapor phase than in the liquid phase, allowing for its separation.

UNESCO Nomenclature: 2209
– Physical Chemistry

Type

Abstract System

Disruption

Foundational

Usage

Widespread Use

Precursors

  • Dalton’s law of partial pressures
  • Avogadro’s law and the concept of the mole
  • Clausius-Clapeyron relation describing vapor pressure dependence on temperature
  • Early studies on solutions and mixtures by scientists like Thomas Graham

Applications

  • fractional distillation of crude oil
  • calculating colligative properties like boiling point elevation
  • design of chemical separation processes
  • predicting vapor-liquid equilibrium in the chemical industry
  • modeling atmospheric aerosols

Patents:

NA

Potential Innovations Ideas

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Related to: Raoult’s law, ideal solution, vapor pressure, partial pressure, mole fraction, physical chemistry, thermodynamics, liquid mixture, volatile, Dalton’s law.

Historical Context

Raoult’s Law for Ideal Solutions

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1890

(if date is unknown or not relevant, e.g. "fluid mechanics", a rounded estimation of its notable emergence is provided)

Related Invention, Innovation & Technical Principles

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