Calculate the vapor pressure of a solution containing 24.5 g of glycerin (C₃H₈O₃) in 135 mL of water at 30.0 °C. The vapor pressure of pure water at this temperature is 31.8 torr. Assume that glycerin is not volatile and dissolves molecularly (i.e., it is not ionic), and use a density of 1.00 g/mL for the water.

A solution contains a mixture of pentane and hexane at room temperature. The solution has a vapor pressure of 258 torr. Pure pentane and hexane have vapor pressures of 425 torr and 151 torr, respectively, at room temperature. What is the mole fraction composition of the mixture? (Assume ideal behavior.)

A solution contains 50.0 g of heptane (C₇H₁₆) and 50.0 g of octane (C₈H₁₈) at 25 °C. The vapor pressures of pure heptane and pure octane at 25 °C are 45.8 torr and 10.9 torr, respectively. Assuming ideal behavior, answer the following: d. Why is the composition of the vapor different from the composition of the solution?

An aqueous solution contains 36% HCl by mass. Calculate the molality and mole fraction of the solution.

Which solution has the highest vapor pressure? a. 20.0 g of glucose (C₆H₁₂O₆) in 100.0 mL of water b. 20.0 g of sucrose (C₁₂H₂₂O₁₁) in 100.0 mL of water c. 10.0 g of potassium acetate KC₂H₃O₂ in 100.0 mL of water