0.0519 kg of biphenyl (C₁₂H₁₀) is dissolve in benzene (C₆H₆) to create a solution with a total volume of 350.0 mL. (Assume the change in volume is negligible)   What intermolecular forces are shared between biphenyl and benzene? If the boiling point of pure benzene is 80.1 °C, then what would be the boiling point of this solution in °C? (Kb for benzene is 2.53 °C/m and the density of benzene is 0.877 g/mL) If the vapor pressure of pure benzene is 24.4 kPa at 40.0 °C, then what will the vapor pressure of the solution be in kPa? (Consider biphenyl to be nonvolatile and the density of benzene is 0.877 g/mL) What would be the osmotic pressure (in atm) of this solution at 40.0 °C? Assume the density of the solution is the same as benzene, 0.877 g/mL.

The solvent carbon disulfide has a melting point of -111.5 deg C, and a freezing point depression constant of 3.83 deg C/m. If you prepare a solution by dissolving 39.0 g of benzene, C6H6 in 500 g of carbon disulfide what would the freezing point of the solution be ?

At what temperature (in °C) will a solution in which 66.28 grams of iron (III) chloride has been added to 1,291 grams of water boil?  The boiling point of water is 100.00°C.  You should use the experimental value of the van't Hoff factor for this calculation.   (5 significant figures)

A solution is made by dissolving 0.0303 kg of biphenyl (C₁₂H₁₀) in 350.0 mL of benzene (C₆H₆).   - What intermolecular forces are shared between biphenyl and benzene?   - If the boiling point of pure benzene is 80.1 °C, then what would be the boiling point of this solution in °C? (Kb for benzene is 2.53 °C/m and the density of benzene is 0.877 g/mL)   - If the vapor pressure of pure benzene is 24.4 kPa at 40.0 °C, then what will the vapor pressure of the solution be in kPa? (Consider biphenyl to be nonvolatile and the density of benzene is 0.877 g/mL)   - What would be the osmotic pressure (in atm) of this solution at 40.0 °C? (The density of benzene is 0.877 g/mL.)