Problem: The normal boiling point of diethyl ether is 34.5°C. A solution containing a nonvolatile solute dissolved in diethyl ether has a vapor pressure of 698 torr at 34.5°C. What is the mole fraction of diethyl ether in this solution?

FREE Expert Solution

The partial pressure of diethyl ether is simply:


Pmixture = P°diethyl ether Xdiethyl ether


The Vapor pressure of pure diethyl ether is equal to the atmospheric pressure (760 torr) since it is at a boiling point.


Calculate the mole fraction :


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Problem Details

The normal boiling point of diethyl ether is 34.5°C. A solution containing a nonvolatile solute dissolved in diethyl ether has a vapor pressure of 698 torr at 34.5°C. What is the mole fraction of diethyl ether in this solution?

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