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Chapter 11: Problem 61

The normal boiling point of diethyl ether is \(34.5^{\circ} \mathrm{C}\) . A solution containing a nonvolatile solute dissolved in diethyl ether has a vapor pressure of 698 torr at \(34.5^{\circ} \mathrm{C} .\) What is the mole fraction of diethyl ether in this solution?

Short Answer

Expert verified
The mole fraction of diethyl ether in the solution is approximately 0.9184.

Step by step solution

01

List the given information

We are given: - Normal boiling point of diethyl ether: \(34.5^{\circ} \mathrm{C}\) - Vapor pressure of the solution: \(698\ torr\) - Atmospheric pressure at normal boiling point: \(760\ torr\)
02

Calculate the mole fraction of diethyl ether

Using the Raoult's Law formula, we can write: \(P_{solution} = (mole\ fraction\ of\ diethyl\ ether) * P^{0}_{diethyl\ ether}\) Now, plug in the given values: \(698\ torr = (mole\ fraction\ of\ diethyl\ ether) * 760\ torr\) Next, solve for the mole fraction of diethyl ether: \(mole\ fraction\ of\ diethyl\ ether = \frac{698\ torr}{760\ torr}\)
03

Calculate the mole fraction

Now, calculate the mole fraction: \(mole\ fraction\ of\ diethyl\ ether = \frac{698}{760} = 0.9184\) The mole fraction of diethyl ether in this solution is approximately 0.9184.

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Most popular questions from this chapter

A solution at \(50^{\circ} \mathrm{C}\) containing 2.0 \(\mathrm{mol}\) of liquid \(\mathrm{A}\) and 3.0 \(\mathrm{mol}\) of liquid \(\mathrm{B}\) has a total vapor pressure of \(240 .\) torr. If pure A has a vapor pressure of 150 . torr at \(50^{\circ} \mathrm{C},\) what is the vapor pres- sure of pure \(\mathrm{B}\) at \(50^{\circ} \mathrm{C} ?\)

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