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Assuming that the solution of gases is ideal, the vapor pressure of the mixture should be:

$\mathbf{Vapor}\mathbf{}{\mathbf{Pressure}}_{\mathbf{mix}}\mathbf{=}\frac{\mathbf{50}\mathbf{}\mathbf{torr}\mathbf{+}\mathbf{85}\mathbf{}\mathbf{torr}}{\mathbf{2}}\phantom{\rule{0ex}{0ex}}\mathbf{Vapor}\mathbf{}{\mathbf{Pressure}}_{\mathbf{mix}}\mathbf{=}\mathbf{67}\mathbf{.}\mathbf{5}\mathbf{}\mathbf{torr}$

A solution is an equimolar mixture of two volatile components A and B. Pure A has a vapor pressure of 50 torr and pure B has a vapor pressure of 100 torr. The vapor pressure of the mixture is 85 torr.

What can you conclude about the relative strengths of the intermolecular forces between particles of A and B (relative to those between particles of A and those between particles of B)?

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Our tutors have indicated that to solve this problem you will need to apply the Solutions, Molarity and Intermolecular Forces concept. You can view video lessons to learn Solutions, Molarity and Intermolecular Forces. Or if you need more Solutions, Molarity and Intermolecular Forces practice, you can also practice Solutions, Molarity and Intermolecular Forces practice problems.

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Based on our data, we think this problem is relevant for Professor Siam's class at PITTSTATE.