Question

A solution of chloroform, CHCl3, and acetone, (CH3)2CO, exhibits a negative deviation from Raoult's law. This result implies that

Answer 1

The given question is incomplete. The complete question is as follows.

A solution of chloroform ($CHCl_{3}$) and acetone ($(CH_{3})_{2}CO$) exhibits a negative deviation from Raoult's law. This result implies that:

chloroform-chloroform interactions are stronger than chloroform-acetone interactions.

chloroform-chloroform interactions are weaker than chloroform-acetone interactions.

acetone-acetone interactions are stronger than chloroform-acetone interactions.

acetone-acetone interactions are weaker than chloroform-acetone interactions

chloroform-chloroform interactions are weaker than chloroform-acetone interactions AND acetone-acetone interactions are weaker than chloroform-acetone interactions.

Explanation:

It is known that when the forces between the particles of the mixture are stronger than the forces between the particles in the pure liquids then negative deviations from Raoult's law are observed.

Hence, when a solution of chloroform ($CHCl_{3}$) and Acetone ($(CH_{3})_{2}CO$) will exhibit a negative deviation from Roult's law.

Then, chloroform-chloroform interactions should be weaker than chloroform-acetone interactions and acetone-acetone interactions must be weaker than Chloroform-Acetone interactions.

thus, we can conclude that for the given situation  chloroform-chloroform interactions are weaker than chloroform-acetone interactions AND acetone-acetone interactions are weaker than chloroform-acetone interactions.