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 A


2.11 mol

Work Step by Step

$R=0.08206\,L\,atm\,mol^{-1}K^{-1}$ $P=10.5\,atm$ $V=5.00\,L$ $T=(30.0+273)\,K=303\,K$ From the ideal gas law, we have $ n=\frac{PV}{RT}=\frac{10.5\,atm\times5.00\,L}{0.08206\,L\,atm\,mol^{-1}K^{-1}\times303\,K}$ $=2.11\,mol$
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