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 6-5 - Calculating a Gas Pressure with the Ideal Gas Equation - Page 206: Practice Example B


$5.59\times10^{14}\, molecules$

Work Step by Step

$T= (25+273)\,K=298\,K$ $R=8.3145\,J\,mol^{-1}K^{-1}$ $P=6.67\times10^{-7}\,Pa$ $V=3.45\,m^{3}$ Using the ideal gas equation, we obtain $n=\frac{PV}{RT}=\frac{6.67\times10^{-7}\,Pa\times3.45\,m^{3}}{8.3145\,J\,mol^{-1}K^{-1}\times298\,K }$ $=9.287\times10^{-10}\,mol$ Number of molecules of $N_{2}$= $=9.287\times10^{-10}\,mol\times6.02214\times10^{23}\,molecules/mol$ $=5.59\times10^{14}\, molecules$
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