Compounds A and B form an ideal solution. The vapor pressure of pure A is P= 72.2 mmHg and a solution with a mole fraction of A of XA= 0.60 has a total vapor pressure of PTot= 59.6 mmHg. What is the vapor pressure of pure B?

8. A solution containing compounds C and D has a total vapor pressure (Potal) of 120 mmHg and the mole fraction of C is 0.25. The vapor pressure of pure D (PS) is 60 mmHg. What is the vapor pressure of pure C (PE)? A) 60 mmHg O B) 105 mmHg C) 140 mmHg D) 180 mmHg O E) 300 mmHg

What is the vapor pressure (in mmHg) of a solution of 18.8 g of CaCl2 in 161.5 g of water at 45.0oC?  Assume complete dissociation.  The vapor pressure of water at 45.0oC is 71.93 mmHg. Your answer should have 4 significant figures.

Concentrated hydrochloric acid contains 1.15 mol HCl dissolved in 3.54 mol H2O. What is the mole fraction of HCl in concentrated hydrochloric acid? What is the molal concentration of HCl? m

What is the vapor pressure of a solution of salt water that contains 3.46 mols of NaCl in 30 mols of water? The vapor pressure of water at 25 °C is 0.0313 atm

A solution is made by dissolving 41.3 g urea (CH4N20), a nonelectrolyte, in 275 g water. Calculate the vapor pressure of this solution at 25°C and 45°C. vapor pressure of water 25°C 23.8 torr 45°C 71.9 torr vapor pressure at 25°C = torr vapor pressure at 45°C = torr

A solution is made using 16.7 percent by mass CH2Cl2 in CHCl3. At 30 °C, the vapor. pressure of pure CH2Cl2 is 490 mm Hg, and the vapor pressure of pure CHCl3 is 260 mm Hg. The normal boiling point of CHCl3 is 61.7 °C. What is the molality of CH2Cl2 in the solution?

Calculate the vapor pressure at 85.0°C of a solution prepared by dissolving 0.400 mol of liquid dibromoethane (C2H4Br2, P° = 127 torr) in 1.80 mol of liquid dibromopropane (C3H6Br2, P° = 173 torr).

Calculate the vapor pressure at 85.0°C of a solution prepared by dissolving 0.250 mol of liquid dibromoethane (C2H4Br2, P° = 127 torr) in 1.80 mol of liquid dibromopropane (C3H6Br2, P° = 173 torr).

A solution made by dissolving 150.0 g of an unknown compound in 425.0 mL of benzene to make a solution which has a freezing point 18.6 °C lower than that of pure benzene. Kf for benzene is 5.12 °C/m and the density of benzene is 0.877 g/mL.     What was the molality of the solution?   How many moles of the unknown compound were dissolved in the solution?   What is the molar mass of the unknown compound?