General Chemistry: Principles and Modern Applications (10th Edition)

Published by Pearson Prentice Hal
ISBN 10: 0132064529
ISBN 13: 978-0-13206-452-1

Chapter 6 - Gases - Example 6-12 - Calculating the Partial Pressures in a Gaseous Mixture - Page 214: Practice Example A


$P_{CO_{2}}=2.47\,atm$ $P_{H_{2}O}= 0.0348\,atm$

Work Step by Step

We find: $P_{CO_{2}}= \frac{n_{CO_{2}}}{n_{total}}\times P_{total}$ $=\frac{0.197}{0.197+0.00278}\times2.50\,atm$ $=2.47\,atm$ $P_{H_{2}O}=\frac{n_{H_{2}O}}{n_{total}}\times P_{total}$ $=\frac{0.00278}{0.197+0.00278 }\times2.50\,atm$ $= 0.0348\,atm$
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