Which law states that the partial pressure of any volatile component of a solution is equal to the vapor pressure of the pure component multiplied by its mole fraction in that solution?

💡 Solution & Explanation

Raoult law governs ideal liquid solutions, stating that the partial vapor pressure of each volatile constituent is proportional to its mole fraction in the liquid phase. Henry law applies to gas solubility in liquids under low concentrations. Dalton law deals with non-reacting gas mixtures in the gaseous state rather than liquid solutions. Graham law describes rates of gas effusion and diffusion relative to molar masses. Ideal solutions obey Raoult law across all proportions of solute and solvent.