Question

How is the vapour pressure of the liquid related to interaction pattern between the molecules of the components of a liquid mixture?? ​

Answer 1

Answer:

A pure liquid experiences a greater amount of vapour pressure as against a liquid's solution. It is inversely proportional to the forces of attraction existing between the molecules of a liquid. It increases with a rise in the temperature. This is because the molecules gain kinetic energy and thus, vapourise briskly.

Answer 2

Explanation:

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If you have a second liquid, the same thing is true. At any particular temperature a certain proportion of the molecules will have enough energy to leave the surface.

In an ideal mixture of these two liquids, the tendency of the two different sorts of molecules to escape is unchanged.

You might think that the diagram shows only half as many of each molecule escaping - but the proportion of each escaping is still the same. The diagram is for a 50/50 mixture of the two liquids. That means that there are only half as many of each sort of molecule on the surface as in the pure liquids. If the proportion of each escaping stays the same, obviously only half as many will escape in any given time. If the red molecules still have the same tendency to escape as before, that must mean that the intermolecular forces between two red molecules must be exactly the same as the intermolecular forces between a red and a blue molecule.