Alcohol aqueous solution can be regarded as ideal dilute solution at 370.26 K, the total vapor pressure of this solution is 101.3 kPa, the mole fraction of alcohol x(alcohol) = 0.03. At %3D the same temperature, the vapor pressure of pure water is 91.3 kPa, please calculate: the vapor partial pressure of alcohol and water above the alcohol aqueous solution when x(alcohol) = 0.02. %3D

Alcohol aqueous solution can be regarded as ideal dilute solution at 370.26 K, the total vapor pressure of this solution is 101.3 kPa, the mole fraction of alcohol x(alcohol) = 0.03. At %3D the same temperature, the vapor pressure of pure water is 91.3 kPa, please calculate: the vapor partial pressure of alcohol and water above the alcohol aqueous solution when x(alcohol) = 0.02. %3D

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

The enthalpy of fusion of solute B is 4,384.28 kJ/mol and its melting point is 870.49oC. Calculate its ideal solubility (nB) in 8.53 moles of solvent at 143.49oC.
What is the vapor pressure above a mixture that is 40% (w/w) ethanol (CH3CH2OH) and 60% (w/w) water at 30ºC? The standard vapor pressure of ethanol and water at that temperature is 78.10 torr and 31.74 torr respectively. Assume these solutions obey Raoult's law.
Calculate the boiling point (Tbp) of an aqueous solution that is 2.222molal sucrose(aq)under standard conditions. Report the value with 4 sig figs.
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
A solution is prepared at 25oC by mixing 20g of K2SO4 with 150mL of water. The density of water at this temperature is 1 g/mL. What is the m of K2SO4. Solve for the m of K2SO4 An aqueous solution of hydrofluoric acid is 12.5 molal with respect to HF and has a density of 1.070 g/mL at 25oC. Calculate the followinga. mole fraction of HFb. %w/w of HFc. molarityd. molalitya. mole fraction of HF
One mole of a component A and twomoles of a component B are mixed at270C to form an ideal binary solution. calculate the Vmix , Gmix Hmix and Smix. Assume that R=8.314 JK1mol-1 ?
An aqueous solution of hydrofluoric acid is 12.5 molal with respect to HF and has adensity of 1.070 g/mL at 25oC. Calculate the following:a. mole fraction of HFb. %w/w of HFc. molarityd. molality
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 total volume of a solution containing compound X with a molar mass of 50, and 1kg of water at 25°C is found to be given by the expression: V (in mL) = 990.64 + 50.464m – 0.315m2 Where m = molality. Calculate the partial molar volume of water (in mL/mol) in a solution prepared by mixing 1kg of water and 491grams of compound X.
Assuming benzene and toluene form ideal solution, what is the mole fraction of toluene in a solution that has a total vapor pressure of 88.98 torr at 20.0oC and 1.0 bar? The vapor pressures of toluene and benzene at 20.0oC and 1.0 bar are 22.14 torr and 75.01 torr, respctively.
A equal mixture of hexane and heptane behaves as an ideal solution. At 25 ◦C , the equilibrium vaporpressure is 0.219 atm for hexane and 0.075 for heptane. What is the equilibrium vapor pressure for atwo-to-one mixture of heptane to hexane?
A student determines the molar mass of acetone, , She found that the equilibrium temperature of a mixture of ice and water was 1.0C on her thermometer. When she added 11.1g of her sample to the mixture, the temperature, after through stirring, fell to -3.0C. She then poured off the solution through a screen into a beaker. The mass of the solution was 90.4g. a. what was the freezing point depression? b. what was the molarity of the acetone? c. how much aceton was in the decanted solution? d. how much water was in the decanted solution? e. how much acetone would there bein a solution containing 1kg of water and acetone at the same concentration as she has in herexperiment? f. what did she find to be the molar mass of aceton, assumingshe made the calculation properly?