1. At 10.4 °C solutions of tetrahydrofuran (THF) and diethyl ether are described as being ideal over the entire range of composition. At this temperature, the vapour pressures of dilute solutions of THF in liquid diethyl ether are as follows: XTHF 0.004 0.009 0.016 PTHF / kPa 9.4 6.6 33.5 (b) At 10.4 °C, the vapour pressure of pure diethyl ether is 300 mmHg and that of THF is 107 mmHg. Calculate the vapour pressure of this solution when 0.06 moles of THF is mixed with 11.1 moles of diethyl ether. Justify the use of any equations used, and state all assumptions.

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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1.
At 10.4 °C solutions of tetrahydrofuran (THF) and diethyl ether are described as being
ideal over the entire range of composition. At this temperature, the vapour pressures of
dilute solutions of THF in liquid diethyl ether are as follows:
XTHF
0.004
0.009
0.016
PTHF / kPa
33.5
6.6
9.4
(b) At 10.4 °C, the vapour pressure of pure diethyl ether is 300 mmHg and that of THF is 107
mmHg. Calculate the vapour pressure of this solution when 0.06 moles of THF is mixed
with 11.1 moles of diethyl ether. Justify the use of any equations used, and state all
assumptions.
Transcribed Image Text:1. At 10.4 °C solutions of tetrahydrofuran (THF) and diethyl ether are described as being ideal over the entire range of composition. At this temperature, the vapour pressures of dilute solutions of THF in liquid diethyl ether are as follows: XTHF 0.004 0.009 0.016 PTHF / kPa 33.5 6.6 9.4 (b) At 10.4 °C, the vapour pressure of pure diethyl ether is 300 mmHg and that of THF is 107 mmHg. Calculate the vapour pressure of this solution when 0.06 moles of THF is mixed with 11.1 moles of diethyl ether. Justify the use of any equations used, and state all assumptions.
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