A and B in a solution exhibit negative deviance from Raoult's law. As a result, molecules of A interact with molecules of B greater strongly than they do with molecules of A or B.
When the solution's overall vapour pressure considerably lower than the comparable vapour pressure in the case of the ideal solution, Raoult's law deviates from the norm in a negative way.
Because the intermolecular attractive interactions between A-A and B-B are weaker than any of those between A-B, the vapour pressure decreases, which is the cause of the negative deviation from Raoult's law.
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