Chemistry 10th Edition

Published by Brooks/Cole Publishing Co.
ISBN 10: 1133610668
ISBN 13: 978-1-13361-066-3

Chapter 14 - Solutions - Exercises - Raoult's Law and Vapor Pressure - Page 545: 40


Partial pressure of acetone= 172 torr. Partial pressure of chloroform= 148 torr.

Work Step by Step

Let $p_{1}$ be the partial pressure of acetone. Given $p_{1}^{0}$= 345 torr and mole fraction, $x_{1}=\frac{n_{1}}{n_{1}+n_{2}}= \frac{0.550 mol}{(0.550+0.550)mol}= 0.5$ Then, using Raoult's law, we have $p_{1}=p_{1}^{0}x_{1}= 345 torr\times0.5\approx 172$ torr. Similarly, let $p_{2}$ be the partial pressure of chloroform. $p_{2}= p_{2}^{0}x_{2}= 295 torr\times \frac{n_{2}}{n_{1}+n_{2}}$= $295 torr \times0.5\approx 148 torr$.
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