It is found that dissolving 5.62 g of a substance in 975 g of carbon disulfide (CS2) at 293 K lowers the freezing point by 0.632 K. Note that Kc = 3.8 K kg mol-1, Keb = 2.37 K kg mol-1, Mm (CS2) = 76.141 g mol-1 and the density of carbon disulfide is 1.26 g cm-3. Calculate the elevation of the boiling point, the ratio of the vapor pressure above the solution to that of the pure solvent, the osmotic pressure and the molecular weight of the solute. P * (CS2) = 0.394 bar at 293 K
It is found that dissolving 5.62 g of a substance in 975 g of carbon disulfide (CS2) at 293 K lowers the freezing point by 0.632 K. Note that Kc = 3.8 K kg mol-1, Keb = 2.37 K kg mol-1, Mm (CS2) = 76.141 g mol-1 and the density of carbon disulfide is 1.26 g cm-3. Calculate the elevation of the boiling point, the ratio of the vapor pressure above the solution to that of the pure solvent, the osmotic pressure and the molecular weight of the solute. P * (CS2) = 0.394 bar at 293 K
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 46P
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It is found that dissolving 5.62 g of a substance in 975 g of carbon disulfide (CS2) at 293 K lowers the freezing point by 0.632 K. Note that Kc = 3.8 K kg mol-1, Keb = 2.37 K kg mol-1, Mm (CS2) = 76.141 g mol-1 and the density of carbon disulfide is 1.26 g cm-3. Calculate the elevation of the boiling point, the ratio of the vapor pressure above the solution to that of the pure solvent, the osmotic pressure and the molecular weight of the solute. P * (CS2) = 0.394 bar at 293 K
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