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D2. We are absorbing hydrogen sulfide at 15.0°C into water. Entering water is pure. Feed gas contains 0.12 mol% H₂S. Recover 97.0% of H₂S in the water. The total gas flow rate is 10.0 kmol/h. Total liquid flow rate is 2000.0 kmol/h. Total pressure is 2.5 atm. You can assume that total liquid and gas flow rates are constant. Equilibrium data are in Table 12-1. a. Calculate the outlet gas and liquid mole fractions of hydrogen sulfide. b. Calculate the number of equilibrium stages required using a McCabe-Thiele diagram. If L/V = M(L/V) min, find multiplier M (M > 1.0). Why is this operation not practical? What would you do to make the process practical? c. d.

D2. We are absorbing hydrogen sulfide at 15.0°C into water. Entering water is pure. Feed gas contains 0.12 mol% H₂S. Recover 97.0% of H₂S in the water. The total gas flow rate is 10.0 kmol/h. Total liquid flow rate is 2000.0 kmol/h. Total pressure is 2.5 atm. You can assume that total liquid and gas flow rates are constant. Equilibrium data are in Table 12-1. a. Calculate the outlet gas and liquid mole fractions of hydrogen sulfide. b. Calculate the number of equilibrium stages required using a McCabe-Thiele diagram. If L/V = M(L/V) min, find multiplier M (M > 1.0). Why is this operation not practical? What would you do to make the process practical? c. d.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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TABLE 12-1. Henry's law constants H for Eq. (12-3) for CO2, CO, and H₂S in water. H is in atm/mole fraction. T°C 0 LO 5 10 15 20 25 30 35 40 45 50 60 70 80 90 100 CO₂ 728 876 1040 1220 1420 1640 1860 2090 2330 2570 2830 3410 CO 35,200 39,600 44,200 48,900 53,600 58,000 62,000 65,900 69,600 72,900 76,100 82,100 84,500 84,500 84,600 84,600 H₂S 268 315 367 423 483 545 609 676 745 814 884 1030 1190 1350 1440 1480
Transcribed Image Text:TABLE 12-1. Henry's law constants H for Eq. (12-3) for CO2, CO, and H₂S in water. H is in atm/mole fraction. T°C 0 LO 5 10 15 20 25 30 35 40 45 50 60 70 80 90 100 CO₂ 728 876 1040 1220 1420 1640 1860 2090 2330 2570 2830 3410 CO 35,200 39,600 44,200 48,900 53,600 58,000 62,000 65,900 69,600 72,900 76,100 82,100 84,500 84,500 84,600 84,600 H₂S 268 315 367 423 483 545 609 676 745 814 884 1030 1190 1350 1440 1480
D2. We are absorbing hydrogen sulfide at 15.0°C into water. Entering water is pure. Feed gas contains 0.12 mol% H₂S. Recover 97.0% of H₂S in the water. The total gas flow rate is 10.0 kmol/h. Total liquid flow rate is 2000.0 kmol/h. Total pressure is 2.5 atm. You can assume that total liquid and gas flow rates are constant. Equilibrium data are in Table 12-1. a. Calculate the outlet gas and liquid mole fractions of hydrogen sulfide. b. Calculate the number of equilibrium stages required using a McCabe-Thiele diagram. c. If L/V = M(L/V) min, find multiplier M (M > 1.0). d. Why is this operation not practical? What would you do to make the process practical?
Transcribed Image Text:D2. We are absorbing hydrogen sulfide at 15.0°C into water. Entering water is pure. Feed gas contains 0.12 mol% H₂S. Recover 97.0% of H₂S in the water. The total gas flow rate is 10.0 kmol/h. Total liquid flow rate is 2000.0 kmol/h. Total pressure is 2.5 atm. You can assume that total liquid and gas flow rates are constant. Equilibrium data are in Table 12-1. a. Calculate the outlet gas and liquid mole fractions of hydrogen sulfide. b. Calculate the number of equilibrium stages required using a McCabe-Thiele diagram. c. If L/V = M(L/V) min, find multiplier M (M > 1.0). d. Why is this operation not practical? What would you do to make the process practical?
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