Chemistry: The Molecular Science (5th Edition)

Published by Cengage Learning
ISBN 10: 1285199049
ISBN 13: 978-1-28519-904-7

Chapter 8 - Properties of Gases - Questions for Review and Thought - Topical Questions - Page 370a: 32


0.90 g

Work Step by Step

Pressure $P=1.1\,atm$ Volume $V=5.0\,L$ Universal gas constant $R= 0.0821\,L\,atm\,mol^{-1}K^{-1}$ Temperature $T=(25\,+273)K= 298\,K$ Recall that $PV=nRT$ (ideal gas law) $\implies $ moles of helium $n= \frac{PV}{RT}$ $=\frac{(1.1\,atm)(5.0\,L)}{(0.0821\,L\,atm\,mol^{-1}K^{-1})(298\,K)}$ $=0.225\,mol$ Mass of helium required= $n\times$ molar mass of helium $=0.225\,mol\times 4.00\,g/mol=0.90\,g$
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