Raoult's law states that the partial pressure of a solvent over a solution is given by the vapor pressure of the pure solvent times the mole fraction of the solvent in the solution.
What is Raoult's law?
- Raoult's law is a physical chemistry relationship that has ramifications for thermodynamics.
- In an ideal combination of liquids, each component's partial pressure is equal to the vapor pressure of the pure component (liquid or solid) multiplied by its mole fraction in the mixture, according to a theory put out by French chemist François-Marie Raoult in 1887.
- As a result, the mole fraction of solute in the solution equals the relative decrease in vapor pressure of a diluted solution of a nonvolatile solute.
- The vapor pressure of the solution will be lower than the vapor pressure of the solvent if a non-volatile solute B (zero vapor pressure, does not evaporate) is dissolved into a solvent A to create an ideal solution.
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