15. 2 Plot the vapour pressure data for a mixture of benzene (B) and ethanoic acid (E) given below and plot the vapour pressure / composition curve for the mixture at 5 0 \ deg C. Then confirm that Raoult's and Henry's laws are obeyed in the appropriate regions. Deduce the activities and activity coefficients of the components on the Raoult's law basis and then, taking B as the solute, its activity and activity coefficient on a Henry's law basis. Finally, evaluate the excess Gibbs energy of the mixture over the composition range spanned by the data. 0 . 0 1 600.0439XE

15. 2 Plot the vapour pressure data for a mixture of benzene (B) and ethanoic acid (E) given below and plot the vapour pressure / composition curve for the mixture at 5 0 \ deg C. Then confirm that Raoult's and Henry's laws are obeyed in the appropriate regions. Deduce the activities and activity coefficients of the components on the Raoult's law basis and then, taking B as the solute, its activity and activity coefficient on a Henry's law basis. Finally, evaluate the excess Gibbs energy of the mixture over the composition range spanned by the data. 0 . 0 1 600.0439XE

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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At 413K the vapor pressure of pure chlorobenzene is 1.237 bar and that of pure bromobenzene is 0.658 bar. These solvents form ideal solutions. A) What is the mole fraction of chlorobenzene in a mixture of these two that just boils at 413K at 1 bar? b) What is the mole fraction of chlorobenzene in the vapor produced in (a)? c) Supposed this vapor is condensed what is its total vapor pressure at 413K?
6. Using phase diagram for the mixtures of benzene and ethylbenzene shown below, estimate: Benzene / Ethybenzene at 1.00 atm By NRTL A) Boiling point of pure ethylbenzene 140- 135- 130- B) Boiling point (Tpp) of solution with molar fraction of benzene 0.3. 125 120- 115 110- C) Composition of vapor phase (molar fractions of both liquids) above the solution with molar fraction of benzene 0.3 at Töp. 105- 100 90 85 80- 75- a1 02 03 04 05 06 0.7 0.8 09 Benzene Mole Fracfioni
2. A benzene (B)-toluene (T) solution is in equilibrium with its vapor at 80°C. If уB -0.670, calculate XB and the total vapor pressure of the solution. The vapor pressures at 80°C of benzene and toluene are 100.4 kPa and 38.7 kPa, respectively. (answer: XB-0.439, P= 65.8 kPa)** Calculate the equilibrium concentration (represented as a mole fraction) of carbon dioxide in fat given that
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The total vapour pressure of an ideal-dilute liquid mixture of acetone and chloroform with a mole fraction of acetone of 0.0500 is 45.08 kPa at 308 K. (a) Use Raou lt's law to determine the partial vapour pressure of acetone for the mixture, given that the vapour pressure of pure acetone is 46.26 kPa at 308 K. (b) Hence calculate the partial vapour pressure of chloroform for the mixture . (c) Determine the Henry's law constant of chloroform at this temperature.(d) The Henry's law constant is lower than the vapour pressureof pure chloroform at 308 K. What does this imply about the nature of the interactions between acetone and chloroform in the liquid mixture?
7. Assume that the data in the table below stems from a liquid mixture that obeys Raoult's law. mole fraction p(MBenzene)/Torr p(Benzene)/Torr Total x(Methylbenzene pressure/Torr 0 0.30 0.45 0.61 0.84 1 0 7.19 (ii) 14.90 (iv) 25.02 80.00 (i) 43.57 (iii) 11.90 a) Estimate the missing values. b) Estimate the total pressure for each composition. c) Determine which component is more volatile
I submitted this question yesterday; the first answer was right, the second was wrong. Please take another look. Thank you! 9.762 g of a non-volatile solute is dissolved in 175.0 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 25°C the vapour pressure of the solution is 23.405 torr.The vapour pressure of pure water at 25°C is 23.756 torr.Calculate the molar mass of the solute (g/mol). answer: 67.0 g/mol -- correct Now suppose, instead, that 9.762 g of a volatile solute is dissolved in 175.0 g of water.This solute also does not react with water nor dissociate in solution.The pure solute displays, at 25°C, a vapour pressure of 2.376 torr.Again, assume an ideal solution.If, at 25°C the vapour pressure of this solution is also 23.405 torr.Calculate the molar mass of this volatile solute. answer: 48.81 g/mol -- wrong Hint: Note that the calculation is greatly simplified if you…
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