The molar mass of a nonelectrolyte is 58.0 g/mol. Compute the boiling point of a solution containing 20.2 g of this compound and 600.0 g of water. The barometric pressure during the experiment was such that the boiling point of pure water was 99.725 °C

A solution containing 0.10 mol of naphthalene (nonvolatile) and 0.90 mol of benzene is cooled until some solid benzene freezes out. The solution is then decanted off from the solid and the decanted solution is warmed to 80°C, at which temperature the vapor pressure above the solution is found to be 670 torr. The normal freezing and boiling points of pure benzene are 5.5 °C and 80°C, respectively and the molar enthalpy of fusion of benzene ∆fus?=10.67 kJ/mol Assume the solution is ideal. a) Calculate the temperature to which the solution was cooled originally. b) Calculate the number of moles of benzene that froze out.

1 for a certain substance X. When 38.6 g of urea (NH,), CO) The molal boiling point elevation constant K, =1.54 °C·kg mol are dissolved in 950. g of X, the 9. 2 solution boils at 113.3 °C. Calculate the boiling point of pure X. Round your answer to 4 significant digits. x10

Given the following mixture of two compounds 50.00 mL of X (MW =78.00 g/mol)(density 1.219 g/mL) and 695.00 mL of Y (65.00 g/mol))(density 1.277 g/mL). The vapor pressure of pure Y is 25.00. Calculate the vapor pressure of the solution.