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-chloroform and 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.
The answer is W. chloroform-chloroform and acetone-acetone interactions are stronger than chloroform-acetone interactions. This is because the bond between acetone-acetone is a dipole-dipole interactions and chloroform-chloroform dipole-dipole compared to the weaker hydrogen-bonding between acetone-chloroform.
It turns out that this hydrogen-bonding happens to be stronger the original dipole-dipole forces, so this shows NEGATIVE DEVIATION from Raoult's law.
Chloroform Chloroform and acetone acetone interactions are stronger than chloroform acetone interactions.
Explanation:
When chloroform and acetone mixed together, it will form a solution with negative deviation from Raoult's law because chloroform form hydrogen bond with acetone molecules. If a vapour mixture is lower that what is expected, negative deviation arises.
