14. Solutions

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.

While mercury is very useful in barometers, mercury vapor is toxic. Given that mercury has a ΔHvap of 59.11 kJ/mol and its normal boiling point is 356.7°C, calculate the vapor pressure in mmHg at room temperature, 25°C.