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.

. 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.

A salt solution has an osmotic pressure of 17.0 atmospheres at 17°C. What assumptions must be made to calculate the freezing point of this solution? molality and molarity of the solution are approximately equal and that the electrolyte is behaving ideally molarity is twice the molality and the electrolyte (salt) is behaving ideally molality and molarity of the solution are approximately equal and there is no electrolyte any more salt is KCl the freezing point is at 0°C

A solution contains a mixture of pentane and hexane at room temperature. Its vapor pressure is 0.3395 atm. Pure pentane and pure hexane have vapor pressures56.66 kPa and 20.13 kPa, respectively. Calculate the composition of the mixturein mole fraction, assuming the solution has an ideal behaviour