A solution contains 3.50 g of a nonvolatile pure hydrocarbon in 95 g acetone. The boiling points of pure acetone and the solution are 55.95°C and 56.50°C, respectively. The molal boiling point constant of acetone is 1.7 1°C-kg/mol. What is the molar mass of the hydrocarbon? Molar massg/mol Submit Answer Try Another Version 5 item attempts remaining

In terms of Raoults law, distinguish between an ideal liquid-liquid solution and a nonideal liquid-liquid solution. lf a solution is ideal, what is true about Hsoln, T for the solution formation, and the interactive forces within the pure solute and pure solvent as compared to the interactive forces within the solution? Give an example of an ideal solution. Answer the previous two questions for solutions that exhibit either negative or positive deviations from Raoults law.

If a volatile solute is added to a volatile solvent, both substances contribute to the vapor pressure over the solution. Assuming an ideal solution, the vapor pressure of each is given by Raoults law, and the total vapor pressure is the sum of the vapor pressures for each component. A solution, assumed to be ideal, is made from 1.0 mol of toluene (C6H5CH3) and 2.0 mol of benzene (C6H6). The vapor pressures of the pure solvents are 22 mm Hg and 75 mm Hg, respectively, at 20 C. What is the total vapor pressure of the mixture? What is the mole fraction of each component in the liquid and in the vapor?

Consider 2 vapor pressure curves A and B. They are the vapor pressure curves of pure benzene and a contaminated solution of benzene with a nonvolatile solute. (a) Which graph shows the vapor pressure curve for pure benzene? (b) What is the boiling point of the contaminated benzene solution? (c) Estimate the molality of the contaminated solution (k b=2.53C/m).