A mixture of chloroform () and acetone () shows a strong negative deviation from Raoult's law. What is the primary molecular reason for this specific macroscopic behavior?

Question

A mixture of chloroform ($CHCl_3$) and acetone ($CH_3COCH_3$) shows a strong negative deviation from Raoult's law. What is the primary molecular reason for this specific macroscopic behavior?

Prashant Kotian · Accepted Answer

Correct answer: B. A negative deviation occurs when solute-solvent (A-B) interactions are stronger than the original solute-solute and solvent-solvent interactions. In the case of and acetone, the hydrogen atom of chloroform forms a strong intermolecular hydrogen bond with the oxygen atom of the acetone carbonyl group, lowering the vapor pressure.

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