10. Compounds C and D form nearly ideal solutions. At 20°C, the vapor pressure of pure C and D are 9.9 kPa and 2.9 kPa, respectively. An equimolar solution of C and D is boiled by reducing the external pressure below the vapor pressure. (Z a. Sketch and label the phase diagram. Calculate the following: b. pressure when boiling begins; c. composition of each component in the vapor; and d. vapor pressure when only a trace of liquid remains. Assume that the rate of vaporization is low enough for the temperature to remain constant.
10. Compounds C and D form nearly ideal solutions. At 20°C, the vapor pressure of pure C and D are 9.9 kPa and 2.9 kPa, respectively. An equimolar solution of C and D is boiled by reducing the external pressure below the vapor pressure. (Z a. Sketch and label the phase diagram. Calculate the following: b. pressure when boiling begins; c. composition of each component in the vapor; and d. vapor pressure when only a trace of liquid remains. Assume that the rate of vaporization is low enough for the temperature to remain constant.
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter16: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 114CP: Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution...
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Transcribed Image Text:10. Compounds C and D form nearly ideal solutions. At 20°C, the vapor pressure of pure C and D are
9.9 kPa and 2.9 kPa, respectively. An equimolar solution of C and D is boiled by reducing the
external pressure below the vapor pressure.
a. Sketch and label the phase diagram.
Calculate the following:
22
b. pressure when boiling begins;
c. composition of each component in the vapor; and
d. vapor pressure when only a trace of liquid remains.
Assume that the rate of vaporization is low enough for the temperature to remain constant.
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