In an ideal solution of liquids A and B, the vapor pressure of a mixture of 1 mole of A and 2 moles of B is 0.5 atm at 70°C. Three moles of A is added to the solution at 70°C and the vapor pressure of the solution rises to 0.7 atm. Calculate what the vapor pressure (in atm) would be if some of the vapor in equilibrium with the first solution were completely condensed.
In an ideal solution of liquids A and B, the vapor pressure of a mixture of 1 mole of A and 2 moles of B is 0.5 atm at 70°C. Three moles of A is added to the solution at 70°C and the vapor pressure of the solution rises to 0.7 atm. Calculate what the vapor pressure (in atm) would be if some of the vapor in equilibrium with the first solution were completely condensed.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter11: Solutions
Section: Chapter Questions
Problem 42P
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![In an ideal solution of liquids A and B, the vapor pressure
of a mixture of 1 mole of A and 2 moles of B is 0.5 atm at
70°C. Three moles of A is added to the solution at 70°C
and the vapor pressure of the solution rises to 0.7 atm.
Calculate what the vapor pressure (in atm) would be if
some of the vapor in equilibrium with the first solution were
completely condensed.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc9db6712-484f-4b2f-b9a6-31db9b80a363%2F403f041c-45e5-4f6e-8866-97e67e29970e%2Fuhiq8ca_processed.png&w=3840&q=75)
Transcribed Image Text:In an ideal solution of liquids A and B, the vapor pressure
of a mixture of 1 mole of A and 2 moles of B is 0.5 atm at
70°C. Three moles of A is added to the solution at 70°C
and the vapor pressure of the solution rises to 0.7 atm.
Calculate what the vapor pressure (in atm) would be if
some of the vapor in equilibrium with the first solution were
completely condensed.
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