Significance of Raoult’s Law
Importance of Raoult’s law can be expressed in terms of following points:
- Raoult’s law helps us to calculate the total vapour pressure of a solution which means the pressure exerted by the vapours on the liquid solvent when they are in equilibrium.
- Raoult’s law is also used to determine vapour pressure of the solution in case of non volatile solutes.
- If partial pressures of components of a solution are known, we can determine the composition of the solution using Raoult’s law.
- Raoult’s law is also used to determine some of the colligative properties of the solution, i.e. the properties which depend on the concentration of solute particles in the solution such as elevation in boiling point, depression in freezing point, etc.
- Raoult’s law can also be applied to ideal gas mixtures.
Raoult’s Law
Raoult’s Law in chemistry relates partial pressures of volatile liquid components to their mole fractions in a liquid solution. It states that the partial pressure of each component in the solution is directly proportional to its mole fraction. Thus, it helps us to calculate the total vapour pressure of the solution. Based on Raoult’s law, liquid solutions are classified as Ideal Solutions and Non-Ideal Solutions.
In this article, we will discuss the definition of Raoult’s law, ideal and non-ideal solutions, Raoult’s law for non-volatile solutes and some solved numerical problems based on Raoult’s law.
Table of Content
- Raoult’s Law Definition
- Raoult’s Law Formula
- Classification of Solutions based on Raoult’s law
- Raoult’s law for Non-Volatile Solutes
- Raoult’s Law with Other Laws
- Significance of Raoult’s Law
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