How many moles of sucrose (342 g/mol) must be added to 552 g of water (18.02 g/mol) to give a solution with 2.0 mm Hg less vapor pressure than pure water at 20 °C? The vapor pressure of pure water at 20 °C is 17.5 mm Hg. I

A solution consists of 0.901 moles of toluene (C7H8) and 0.600 moles of cyclohexane (C6H12).  The vapor pressures of toluene and cyclohexane at 25oC are 28.4 mmHg and 107.5 mmHg, respectively.  What is the mole fraction of toluene in the vapor above this solution at 25oC?

What would be the theoretical freezing point of a solution made by dissolving 5.444 g of CaSO 4 in 140.0 g of water? The freezing point constant of water is 1.86 °C/molal. The molar mass of CaSO 4 is 136.14 g/mol.     -0.8291 °C     -0.6091 °C     1.063 °C     0.9412 °C     -1.063 °C

A solution is prepared by adding 101 g of lactose (milk sugar) to 102 g of water at 55 °C. The partial pressure of water above the solution is __________ torr. The vapor pressure of pure water at 55 °C is 118 torr.  The MW of lactose is 342.3 g/mol.

Calculate the freezing point of a solution containing 25.0 g. of ClF3 (MM = 92.45 g/mol) in 450. g. of water. The Kf of water is 1.86 °C/m. The freezing point of pure water is 0 ºC.

23. An ethylene glycol solution contains 28.3 g of ethylene glycol, C2H602 in 97.2 mL of water. Calculate the freezing point of the solution. The density of water 1.00 g/mL.

A solution made by dissolving 1.094 g of an unknown nonelectrolyte in 27.386 g of camphor. has a freezing point of 162.1 °C. What is the molar mass of the unknown?       (For camphor Tf = 178.4 °C, and Kf = 37.7 °C/m)

A solution is prepared by adding 5.0 moles of LINO3 to 50.0 mole of water at 25 °C. Pure water has a vapor pressure of 24.0 torr at this temperature. What is the vapor pressure of the solution (torr)?

At a certain temperature the vapor pressure of water is 25.0 torr. A glucose solution is prepared by mixing 5.00 g of glucose and 2.00 moles of water. What is the expected vapor pressure of the solution? Molar mass of water = 18.02 g/mol and molar mass of glucose = 180.2 g/mol a) 0.342 torr b) 3.05 torr c) 22.0 torr d) 24.7 torr

The liquid used in automobile cooling systems is prepared by dissolving ethylene glycol (HOCH2CH2OH) in water. Ethylene glycol has a molar mass of 62.07 g/mol and a density of 1.115 g/mL at 50.0°C.Calculate the vapor pressure at 50°C of a coolant solution that is 55.0:45.0 ethylene glycol-to-water by volume. At 50.0°C, the density of water is 0.9880 g/mL, and its vapor pressure is 92 torr. The vapor pressure of ethylene glycol is less than 1 torr at 50.0°C.