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A dilute solution of bromine behaves ideally with a non-polar solvent at 300K. The Henry's law constant for Br₂ in this solution, when expressed using mole fraction “units”, is 150 torr. The mole fraction of Br₂ in the solution is 0.05 and the vapor pressure of the pure solvent is 50 torr at 300K. Calculate the following assuming the solution behaves as an ideal dilute solution at 300K. i) the vapor pressure of each component ii) the total gas-phase pressure iii) the composition of the vapor phase in mole fractions

A dilute solution of bromine behaves ideally with a non-polar solvent at 300K. The Henry's law constant for Br₂ in this solution, when expressed using mole fraction “units”, is 150 torr. The mole fraction of Br₂ in the solution is 0.05 and the vapor pressure of the pure solvent is 50 torr at 300K. Calculate the following assuming the solution behaves as an ideal dilute solution at 300K. i) the vapor pressure of each component ii) the total gas-phase pressure iii) the composition of the vapor phase in mole fractions

Principles of Modern Chemistry
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 74AP
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A dilute solution of bromine behaves ideally with a non-polar solvent at 300K. The Henry's law constant for Br₂ in this solution, when expressed using mole fraction "units", is 150 torr. The mole fraction of Br₂ in the solution is 0.05 and the vapor pressure of the pure solvent is 50 torr at 300K. Calculate the following assuming the solution behaves as an ideal dilute solution at 300K. i) the vapor pressure of each component ii) the total gas-phase pressure iii) the composition of the vapor phase in mole fractions
Transcribed Image Text:A dilute solution of bromine behaves ideally with a non-polar solvent at 300K. The Henry's law constant for Br₂ in this solution, when expressed using mole fraction "units", is 150 torr. The mole fraction of Br₂ in the solution is 0.05 and the vapor pressure of the pure solvent is 50 torr at 300K. Calculate the following assuming the solution behaves as an ideal dilute solution at 300K. i) the vapor pressure of each component ii) the total gas-phase pressure iii) the composition of the vapor phase in mole fractions
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