3.(a) At 10 °C, the vapour pressures of pure chloroform (CHCI3) and pure dichloromethane(CH2C12) are 101 mmHg and 235 mmHg, respectively. Assume that a solution made bymixing CHCI3 and CH2C12 is ideal.i. If the vapour pressure of the resulting solution is 140 mmHg and it contains 1.25moles of components, what is the mass of CHCI3 present in that solution.

Given: Partial pressure of CHCl3 = 101 mmHg Partial pressure of CH2Cl2 = 235 mmHg Total pressure of…

(CH2C12) are 101 mmHg and 235 mmHg, respectively. Assume th mixing CHCI3 and CH2C12 is ideal. i. If the vapour pressure of the resulting solution is 140 mmH moles of components, what is the mass of CHC13 present in

(CH2C12) are 101 mmHg and 235 mmHg, respectively. Assume th mixing CHCI3 and CH2C12 is ideal. i. If the vapour pressure of the resulting solution is 140 mmH moles of components, what is the mass of CHC13 present in

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

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Question

3.
(a) At 10 °C, the vapour pressures of pure chloroform (CHCI3) and pure dichloromethane
(CH2C12) are 101 mmHg and 235 mmHg, respectively. Assume that a solution made by
mixing CHCI3 and CH2C12 is ideal.
i. If the vapour pressure of the resulting solution is 140 mmHg and it contains 1.25
moles of components, what is the mass of CHCI3 present in that solution.

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