6. The vapour pressure of water and propanol are 71.9 and 74.0 torr respectively. The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various compositions, with the following data collected at 45°C: Vapour Pressure (torr) XH20 74.0 0.15 77.3 a) Are solutions of water and propanol ideal, or a positive or negative deviation from Raoult's Law? Explain. b) Predict the sign of AHsoln for water-propanol solutions. 0.37 80.2 0.54 81.6 c) Are the interactive forces between propanol and water molecules weaker than, stronger than, or equal to the interactive forces between the pure substances? Explain. 0.69 80.6 0.83 78.2 1.00 71.9 d) Which of the solutions in the data would have the lowest normal boiling point?

6. The vapour pressure of water and propanol are 71.9 and 74.0 torr respectively. The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various compositions, with the following data collected at 45°C: Vapour Pressure (torr) XH20 74.0 0.15 77.3 a) Are solutions of water and propanol ideal, or a positive or negative deviation from Raoult's Law? Explain. b) Predict the sign of AHsoln for water-propanol solutions. 0.37 80.2 0.54 81.6 c) Are the interactive forces between propanol and water molecules weaker than, stronger than, or equal to the interactive forces between the pure substances? Explain. 0.69 80.6 0.83 78.2 1.00 71.9 d) Which of the solutions in the data would have the lowest normal boiling point?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.84QE

See similar textbooks

Similar questions

Some nonelectrolyte solute (molar mass = 142 g/mol) was dissolved in 150. mL of a solvent (density = 0.879 g/cm3). The elevated boiling point of the solution was 355.4 K. What mass of solute was dissolved in the solvent? For the solvent, the enthalpy of vaporization is 33.90 kJ/mol, the entropy of vaporization is 95.95 J/K mol, and the boiling-point elevation constant is 2.5 K kg/mol.
The vapour pressure of mercury at 20 °c is 160 mPa; what is its vapour pressure at 40 °c given that its enthalpy of vaporization is 59.30 kJ mol-1?
C6H5Cl e C6H5Br form nearly ideal mixtures. At 136.7◦ C the vapor pressure of C6H5Cl is 1.137 bar, while that of C6H5Br is 0.604 bar. Which is the composition of the mixture for which the total vapor pressure is 1 bar ?
1,1-Dichloroethane (CH3CHCl2) has a vapour pressure of 228 torr at 25 °C; at the same temperature, 1,1-dichlorotetrafluoroethane (CF3CCl2F) has a vapour pressure of 79 torr. What mass of 1,1-dichloroethane must be mixed with 240.0 g of 1,1-dichlorotetrafluoroethane to give a solution with vapour pressure 157 torr at 25 °C? Assume ideal behaviour. (1 atm = 760 torr).
Predict the partial vapour pressure of HCl above its solution in liquid germanium tetrachloride of molality 0.10 mol kg−1. For data, see Exercise E5A.8(a).
Consider a pure liquid in equilibrium with its vapor at constant temperature. a) write an expression relating the chemical potential of the liquid, u(l), and vapor, u(g). b) express u(g) in terms of the vapor pressure of the pure liquid, P.
Ethylene glycol is used as an antifreeze to lower the freezing point of water in automotive engines in the winter. If the heat of fusion of water is 6003 J/mol and that of ethylene glycol is 10,998 J/mol, compute and plot (on the same graph) the following as a function of water mole fraction, xH2O:a. The freezing points of ethylene glycol-in-water mixturesb. The freezing points of water-in-ethylene glycol mixturesFor the purpose of this problem, you may assume ideal solutions. From the above analysis, what would be your recommendation to an automotive manufacturer regarding the molar composition of water and ethylene glycol to ensure the lowest possible freezing point? What would you estimate the corresponding freezing point to be?
For a benzene (C6H6) toluene (C6H5CH3) mixture, at 120 °C, the following values are obtained for the total vapour pressures of the given mixtures:
At 25°C, 0.45 mol of the non-volatile solute glucose (C6H12O6) is added to 500g of water. At 25°C, the vapour pressure of pure water is 23.8 torr.If the solution is made to freeze, determine its vapour pressure and freezing point. It's given that the normal freezing point of water is 0°C, Kf = 1.86 °C/m, water density is 1g/mL, and the molar mass (g/mol) is C = 12, H = 1, O = 16.
What mass of non volatile solute sucrose needs to be dissolved in 100g of water in order to decrease vapour pressure of water by 25% ?
The osmotic pressu re of an aqueous solution of urea at 300 K is 150 kPa. Calculate the freezing point of the same solution.
The partial molar volumes of two liquids A and B in a mixture in which the mole fraction of A is 0.3713 are 188.2 cm3 mol−1 and 176.14 cm3 mol−1, respectively. The molar masses of the A and B are 241.1 g mol−1 and 198.2 g mol−1. What is the volume of a solution of mass 1.000 kg?