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The vapor pressure of carbon tetrachloride, CCI4, is 0.354 atm, and the vapor pressure of chloroform, CHCI, is 0.526 atm at 316 K. A solution is prepared from equal masses of these two compounds at this temperature. Calculate the mole fraction of the chloroform in the vapor above the solution. If the vapor above the original solu- tion is condensed and isolated into a separate flask, what will the vapor pressure of chloroform be above this new solution?

The vapor pressure of carbon tetrachloride, CCI4, is 0.354 atm, and the vapor pressure of chloroform, CHCI, is 0.526 atm at 316 K. A solution is prepared from equal masses of these two compounds at this temperature. Calculate the mole fraction of the chloroform in the vapor above the solution. If the vapor above the original solu- tion is condensed and isolated into a separate flask, what will the vapor pressure of chloroform be above this new solution?

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter11: Solutions And Colloids
Section: Chapter Questions
Problem 65E: The vapor pressure of methanol, CH3OH, is 94 torr at 20 C. The vapor pressure of ethanol, C2H5OH, is...
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The vapor pressure of carbon tetrachloride, CCI4, is 0.354 atm, and the vapor pressure of chloroform, CHCI, is 0.526 atm at 316 K. A solution is prepared from equal masses of these two compounds at this temperature. Calculate the mole fraction of the chloroform in the vapor above the solution. If the vapor above the original solu- tion is condensed and isolated into a separate flask, what will the vapor pressure of chloroform be above this new solution?
Transcribed Image Text:The vapor pressure of carbon tetrachloride, CCI4, is 0.354 atm, and the vapor pressure of chloroform, CHCI, is 0.526 atm at 316 K. A solution is prepared from equal masses of these two compounds at this temperature. Calculate the mole fraction of the chloroform in the vapor above the solution. If the vapor above the original solu- tion is condensed and isolated into a separate flask, what will the vapor pressure of chloroform be above this new solution?
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