Raoult's law is the expression for the vapor pressure i of component i in an ideal solution io where i is the mole fraction of component i and io the vapor pressure of the pure substance i.
A law that describes the relationship between the vapor pressure of a solution, the mole fraction of the solute, and the vapor pressure of the solute.
Raoult's law is the expression for the vapor pressure A of component A in an ideal solution, viz., Ao where A is the mole fraction of component A and Ao the vapor pressure of the pure substance A.
a dissolved substance will lower the partial pressure of the solvent proportionally to the mole fraction of the dissolved substance. Useful phenomena for the calibration of humidity sensors.
The vapor pressure of a solvent in an ideal solution decreases as its mole fraction decreases.
The vapor pressure of a solvent in an ideal solution equals the mole fraction of the solvent times the vapor pressure of the pure solvent.
Physical law relating the change in vapor pressure of a liquid to the amount of solute dissolved in it. The law states that = , where is the mole fraction of the dissolved solute. The quantity is sometimes referred to as the vapor tension of the solution. Consequences of Raoult's law are the so-called colligative properties of solutions, that is, the depression of freezing and melting points of solutions relative to those of the pure solvent and osmotic pressure. Raoult's law is observed in everyday situations every winter when we put salt on sidewalks to melt the ice. This is simply a depression of the melting point associated with the dissolution of salt in water.