Ammonia is stripped from a dilute aqueous solution by countercurrent contact with air in a column containing seven sieve trays. The equilibrium relationship is ye = 0.80 xe, and when the molar flow of air is 1.5 times that of the solution, 90% of the ammonia is removed. (a) How many ideal stages does the column have and what is the stage efficiency? (b) Under what thermodynamic conditions (temperature, pressure) is the column operating? [Discuss]

Ammonia is stripped from a dilute aqueous solution by countercurrent contact with air in a column containing seven sieve trays. The equilibrium relationship is ye = 0.80 xe, and when the molar flow of air is 1.5 times that of the solution, 90% of the ammonia is removed. (a) How many ideal stages does the column have and what is the stage efficiency? (b) Under what thermodynamic conditions (temperature, pressure) is the column operating? [Discuss]

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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(b) CMC of a surfactant in water at 25 °C is 0.5 g L-¹ and at 45 °C is 0.3 g L-1. The molar mass of the surfactant is 110 g mol-¹. (i) Calculate: The Gibbs energy of micellisation, AGO, of the surfactant at 25 °C and 45 °C, The fractions (%) of the surfactant molecules in free and in micellar states in 0.5 g L-¹ aqueous solution of the surfactant and temperature 45 °C. ● ● (ii) Calculate CMC for the surfactant in water at 55 °C.
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A saturated solution of copper(ll) sulfate, with excess of the solid, is present in equilibrium with its vapour in a closed vessel. (a) How many phases and components are present? (b) How many degrees of freedom are available, and what are they?
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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?
Show that the equation below holds for the definition of ideal gas