The normal boiling point of methanol is 64.7°C. A solution containing a nonvolatile solute dissolved in methanol has a vapor pressure of 417.0 torr at 64.7°C. What is the mole fraction of methanol in this solution?

A solution is prepared by dissolving 0.5 mol of a non-volatile solute in 1.0 mol of water. Calculate the vapor pressure of water above this solution at 338 K, given that the vapor pressure of pure water at this temperature is 0.2467 atm.

Using Raoult's Law, calculate the vapor pressure of water at 50.0°C if the pure vapor pressure of water at this temperature is 12.3 kPa and a non-volatile solute is added to form a solution with a mole fraction of water of 0.8.

Methanol has a normal boiling point of 64.6°C and a heat of vaporization of 35.2 kJ/mol. What is the vapor pressure of methanol at 12.0°C?

The colligative molality of seawater is approximately 1.10 m. Calculate the vapor pressure of seawater at 20 °C. The vapor pressure of pure water at 20 °C is 17.54 Torr. What is the vapor pressure of seawater?

Using Raoult's Law, calculate the vapor pressure of SiCl4 at 33.5 °C given that its vapor pressure is 100 mm Hg at 5.4 °C and ΔHvap = 30.2 kJ/mol.

Using Raoult's Law and the Clausius-Clapeyron equation, what is the vapor pressure of SiCl4 in mmHg at 31.0 °C, given that its vapor pressure is 100 mmHg at 5.4 °C and ΔHvap is 30.2 kJ/mol?

What is the vapor pressure of a 45.0% solution of glucose (C6H12O6) at a particular temperature, given that the vapor pressure of pure water at that temperature is 486 mm Hg?

What is the vapor pressure of a solution made by dissolving 150.0 grams of sucrose (C12H22O11) in 250.0 grams of water at 25.0 °C? The molar mass of sucrose is 342.34 g/mol, the molar mass of water is 18.02 g/mol, and the vapor pressure of pure water at 25.0 °C is 23.8 mmHg.