A solution contains equal amounts (in moles) of liquid components A and B. The v

Question

A solution contains equal amounts (in moles) of liquid components A and B. The vapor pressure of pure A is 100 mmHg and that of pure B is 200 mmHg. The experimentally measured vapor pressure of the solution is 120 mmHg. What are the relative strengths of the solute-solute, solute-solvent, and solvent-solvent interactions in this solution? The intermolecular forces between particles A and B are weaker than those between particles of A and those between particles of B. The intermolecular forces between particles A and Bare stronger than those between particles of A and those between particles of B. The intermolecular forces between particles A and B are the same as those between particles of A and those between particles of B. Nothing can be concluded about the relative strengths of intermolecular forces from this observation. Explain your opinion.

Explanation / Answer

As the vapour pressure increases the interactions will less.

So vapour pressure is inversly proportional to molecular interactions.

Since the vapour pressure of B is more so the molecular interactions are less in B.

The vapour pressure of mixture solution is more than that of A And less than that of B so the intermolecular forces between A and B are stronger than that of particals A and individual B

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