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?

A solution contains naphthalene (C10H8) dissolved in hexane (C6H14) at a concentration of 16.65% naphthalene by mass. Calculate the vapor pressure at 25°C of hexane above the solution. The vapor pressure of pure hexane at 25°C is 151 torr. What is the vapor pressure of hexane above the solution?

A solution is prepared by dissolving 40.0 g of sucrose, C12H22O11, in 250. g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of pure water at 25°C is 23.76 mm Hg?

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.

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?

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?

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?