Vapour Pressure of Solutions of Non-Volatile or Volatile Solutes 14.356 g of a non-volatile solute is dissolved in 265.0 g of water. The solute does not react with water nor dissociate in solution. Assume that the resulting solution displays ideal Raoult's law behaviour.. At 20°C the vapour pressure of the solution is 17.396 torr. The vapour pressure of pure water at 20°C is 17.535 torr. Calculate the molar mass of the solute (g/mol). See example 17.1 on pp718-9 of Zumdahl "Chemical Principles" 8th ed. 1pts Submit Answer Tries 0/5 Now suppose, instead, that 14.356 g of a volatile solute is dissolved in 265.0 g of water. This solute also does not react with water nor dissociate in solution. The pure solute displays, at 20°C, a vapour pressure of 1.754 torr. Again, assume an ideal solution. If, at 20°C the vapour pressure of this solution is also 17.396 torr. Calculate the molar mass of this volatile solute. cf p 719 of Zumdahl "Chemical Principles" 8th ed.

Non-ideal solutions exhibit either positive or negative deviations from Raoult’s law. What are these deviations and how are they caused?

The Rast camphor method is a cryoscopic technique for molar mass determination. Exactly 1.00 g of an isoprenoid of known formula (C5H8)n was dissolved in 5.00 g of camphor. The freezing point of the resulting solution decreased by 27.7 ℃ relative to pure camphor. Knowing that the Kf of camphor is 37.7 deg·kg/mol: Calculate for the molar mass of the isoprenoid. Calculate the value of n in the given formula of the isoprenoid. Report in whole number. The normal freezing point of camphor is 178.4 ℃. At what temperature did the isoprenoid-camphor solution freeze?

2. A and B form an ideal solution. At a total pressure of 0.90 bar, Xa(1)=0.65, XA(g) = 0.45. Using this information, calculate the vapor pressures of pure A and pure B.

A solution is made by dissolving 33.5g of urea (H₂NCONH₂, a non-volatile non-electrolyte) in 310g of water. Calculate the vapour pressure of this solution at 50°C. (note the vapour pressure of pure water at 50°C is 92.5 torr.)

. The vapor pressure of benzene is 10 kPa while methylbenzene is 2.8 kPa. Determine the total pressure of an equimolar solution.

33. 1.18 g aniline liquid is mixed with 1.00 g benzene liquid at 25 oC.  Calculate the mole fraction of aniline in the vapor phase.  At 25 oC, the vapor pressure of pure benzene is 30.5 kPa and the vapor pressure of pure aniline is 28.0 kPa.    molar masses:  benzene = 78.00 g/mole and aniline = 93.12 g/mole  Group of answer choices 0.522 0.233 0.821 0.476

A certain dilute solution has an osmotic pressure of 11.1 atm at 25°C. Calculate the difference between the chemical potential of the solvent in the solution and that of pure water. Assume that the density is the same as that of water at 25°C, 0.99705 g-cm-3. (Hint: Express the chemical potential in terms of mole fraction, x1, and rewrite the osmotic pressure equation as OV = n2RT, where n2 is the number of moles of the solute and V = 1.00 L.)

What is the molar ratio of 1,1-dichloroethane (11DCE) to 1,2-dichloroethane (12DCE) in the gas phase above the solution containing 10 mol of 1,1-dichloroethane and 10 mol of 1,2-dichloroethane at 20oC. The vapor pressure of 1,1-dichloroethane is 24.0 kPa and the vapor pressure of 1,2-dichloroethane is 8.0 kPaat 20oC.

3. (a) At 10 °C, the vapour pressures of pure chloroform (CHCI3) and pure dichloromethane (CH2C12) are 101 mmHg and 235 mmHg, respectively. Assume that a solution made by mixing CHCI3 and CH2C12 is ideal. i. If the vapour pressure of the resulting solution is 140 mmHg and it contains 1.25 moles of components, what is the mass of CHCI3 present in that solution.