Define the terms in Raoult’s law. Figure 10-9 illustrates the net transfer of water molecules from pure water to an aqueous solution of a nonvolatile solute. Explain why eventually all of the water from the beaker of pure water will transfer to the aqueous solution. If the experiment illustrated in Fig. 10-9 was performed using a volatile solute, what would happen? How do you calculate the total vapor pressure when both the solute and solvent are volatile?

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Interpretation Introduction Interpretation: The explanation for the given has to be defined via Raoult’s law. Concept Introduction: Raoult’s law for ideal solution states that the mole fraction of the solvent is directly proportional to the vapor pressure of an ideal solution. Raoult’s law can be expressed by the equation, P solution =χ solvent P° solvent Where, P solution = observed vapor pressure of the solution χ solvent = mole fraction of solvent P° solvent = vapor pressure of pure solvent Explanation To define Raoult’s law Raoult’s law for ideal solution states that the mole fraction of the solvent is directly proportional to the vapor pressure of an ideal solution. Raoult’s law can be expressed by the equation, P solution =χ solvent P° solvent Where, P solution = observed vapor pressure of the solution χ solvent = mole fraction of solvent P° solvent = vapor pressure of pure solvent To state the reason behind why all water from the beaker of pure water will transfer to the aqueous beaker. When the vapor pressure equilibrium P H 2 O is reached, the beaker containing Water will stop having total transfer of Water molecules beyond the beaker. This will never happen. The beaker containing the solution needs an equilibrium vapor pressure of P H 2 O that is less than P H 2 o

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Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Interpretation Introduction

Interpretation: The explanation for the given has to be defined via Raoult’s law.

Concept Introduction:

Raoult’s law for ideal solution states that the mole fraction of the solvent is directly proportional to the vapor pressure of an ideal solution. Raoult’s law can be expressed by the equation,

Psolution=χsolventP°solvent

Where, Psolution = observed vapor pressure of the solution

χsolvent = mole fraction of solvent

P°solvent = vapor pressure of pure solvent

Explanation of Solution

To define Raoult’s law

Raoult’s law for ideal solution states that the mole fraction of the solvent is directly proportional to the vapor pressure of an ideal solution. Raoult’s law can be expressed by the equation,

Psolution=χsolventP°solvent

Where, Psolution = observed vapor pressure of the solution

χsolvent = mole fraction of solvent

P°solvent = vapor pressure of pure solvent

To state the reason behind why all water from the beaker of pure water will transfer to the aqueous beaker.

When the vapor pressure equilibrium PH2O is reached, the beaker containing Water will stop having total transfer of Water molecules beyond the beaker. This will never happen. The beaker containing the solution needs an equilibrium vapor pressure of PH2O that is less than PH2o

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

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