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Chapter 12: Problem 75

These compounds are liquid at \(-10^{\circ} \mathrm{C}\); their boiling points are given: butane, \(-0.5^{\circ} \mathrm{C}\); ethanol, \(78.3^{\circ} \mathrm{C}\); toluene, \(110.6^{\circ} \mathrm{C}\). At \(-10^{\circ} \mathrm{C}\), which of these liquids would you expect to have the highest vapor pressure? Which the lowest?

Short Answer

Expert verified
At \(-10^{\circ} \mathrm{C}\), ethanol would have the highest vapor pressure and toluene would have the lowest vapor pressure.

Step by step solution

01

Identify the Boiling Points

Given, the boiling points of the liquids are: butane (\(-0.5^{\circ} \mathrm{C}\)), ethanol (\(78.3^{\circ} \mathrm{C}\)) and toluene (\(110.6^{\circ} \mathrm{C}\)).
02

Compare the Boiling Points with the Given Temperature

The temperature is given as \(-10^{\circ} \mathrm{C}\). Butane has a boiling point above this temperature, while ethanol and toluene have boiling points below that temperature. So, butane will be a gas and the other two will be liquids.
03

Determine Vapor Pressure Based on Boiling Points

At a given temperature, substances with lower boiling points have higher vapor pressures and those with higher boiling points have lower vapor pressures. So, given that ethanol and toluene are the liquids at \(-10^{\circ} C\), ethanol, with the lower boiling point, will have the higher vapor pressure and toluene, with the higher boiling point, will have the lower vapor pressure. Butane, being a gas, does not come into consideration.

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