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(a)
Interpretation:
The vapor pressure of the solvent in an aqueous solution of 40oC in which the mole fraction of glucose is 0.0316 has to be calculated.
Concept Introduction:
The equilibrium between a liquid and its vapor produces a characteristic vapor pressure for each substance that depends on the temperature. The lowering of the vapor pressure is caused by a lesser ability of the solvent to evaporate, so equilibrium is reached with a smaller concentration of the solvent in the gas phase. The vapor pressure of a solution is expressed using Raoult’s law:
Psolv=χsolvPosolv
The vapor pressure of the solvent (Psolv) above a dilute solution is equal to the mole fraction of the solvent (χsolv) times the vapor pressure of the pure solvent (Posolv).
Mole fraction: Mole fraction of a substance in a solution is the number of moles of that substance divided by the total number of moles of all substances present. The formula is,
χA=Moles of A (in mol)Moles of A (in mol) +Moles of B (in mol) +Moles of C (in mol) +...χA=Moles of A (in mol)Total number of moles of components (in mol)
(b)
Interpretation:
The vapor pressure of the solvent in an aqueous solution of 23oC in which the concentration of urea is 0.0.240 M has to be calculated.
Concept Introduction:
Refer to part (a).
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Chapter 5 Solutions
Chemical Principles: The Quest for Insight
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