Amixture of CH₂Cl₂ (A) and CHCl3 (B) with XA = 0.373 has a total vapor pressure of 0.245 bars at 250 K and the mole fraction of CH₂Cl₂ (A)in the vapor phase is yд = 0.427. Given that the vapor pressure of pure CH₂Cl₂ at 250 K is 0.288 bars, calculate the activity of CH₂Cl₂ in thismixture. Assume that the vapor behaves as an ideal gas.

Given: mole fraction of CH2Cl2 in vapor phase: yA=0.427xA=0.373 Total vapor pressure = 0.288 barsFrom Modified form of Raoult's: Activity coefficient is given by, YA=yAPxAPA*Where, YA=activity coefficient yA=mole fraction of CH2Cl2 in vapor phase xA=mole fraction of CH2Cl2 in liquid phase P=total pressure PA*=Vapor pressure of pure CH2Cl2 Calculation for Activity coefficient: YA=yAPxAPA*YA=0.427×0.245 bar0.373×0.288 barYA=0.974Calculation for activity of CH2Cl2: αA=YAxAαA=0.974×0.373αA=0.363

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A mixture of CH₂Cl₂ (A) and CHCl3 (B) with XA = 0.373 has a total vapor pressure of 0.245 bars at 250 K and the mole fraction of CH₂Cl₂ (A) in the vapor phase is yA = 0.427. Given that the vapor pressure of pure CH₂Cl₂ at 250 K is 0.288 bars, calculate the activity of CH₂Cl₂ in this mixture. Assume that the vapor behaves as an ideal gas.

A mixture of CH₂Cl₂ (A) and CHCl3 (B) with XA = 0.373 has a total vapor pressure of 0.245 bars at 250 K and the mole fraction of CH₂Cl₂ (A) in the vapor phase is yA = 0.427. Given that the vapor pressure of pure CH₂Cl₂ at 250 K is 0.288 bars, calculate the activity of CH₂Cl₂ in this mixture. Assume that the vapor behaves as an ideal gas.

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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Question

A
mixture of CH₂Cl₂ (A) and CHCl3 (B) with XA = 0.373 has a total vapor pressure of 0.245 bars at 250 K and the mole fraction of CH₂Cl₂ (A)
in the vapor phase is yд = 0.427. Given that the vapor pressure of pure CH₂Cl₂ at 250 K is 0.288 bars, calculate the activity of CH₂Cl₂ in this
mixture. Assume that the vapor behaves as an ideal gas.

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