A solution of chloroform (CHCl3) and acetone((CH3)2CO) exhibits a negative deviation from Raoult's law. This result implies that: W. chloroform-chloroform and acetone-acetone interactions are stronger than chloroform-acetone interactions. X. chloroform-chloroformand acetone-acetone interactions are weaker than chloroform-acetone interactions. Y. acetone-acetone interactions are stronger than chloroform-chloroform interactions. Z. acetone-acetone interactions are weaker than chloroform-chloroform interactions.

Raoult's law states, In a solution, vapor pressure is equal to the sum of the vapor pressures of individual component and this implies when it is multiplied by the mole fraction of that component in the solution. Raoult's Law is expressed by the formula:

P solution = Χ solvent [tex]\times[/tex] P0 solvent.

Raoult's law assumes that the components in the mixture are ideal, it assumes that the Chloroform-Chloroform interactions, Chloroform-Acetone, and Acetone-Acetone are the same. A negative deviation is shown by the measurement of observed vapor pressure which is less than that of calculated. Hence the interaction of Chloroform-Chloroform is weaker than the Chloroform-Acetone interactions.