## Chemistry: The Molecular Science (5th Edition)

Published by Cengage Learning

# Chapter 8 - Properties of Gases - Questions for Review and Thought - Topical Questions - Page 370a: 31

#### Answer

$2.6\times10^{3}\,mL$

#### Work Step by Step

Pressure $P=730.\, mmHg\times\frac{1\,atm}{760\, mmHg}$ $=0.9605\,atm$ Number of moles $n=\frac{4.4\,g}{44.0\,g/mol}=0.10\,mol$ Universal gas constant $R= 0.0821\,L\,atm\,mol^{-1}K^{-1}$ Temperature $T=(27\,+273)K= 300.\,K$ Recall that $PV=nRT$ (ideal gas law) $\implies$ Volume $V= \frac{nRT}{P}$ $=\frac{(0.10\,mol)(0.0821\,L\,atm\,mol^{-1}K^{-1})(300.\,K)}{0.9605\,atm}$ $=2.6\,L=2.6\times10^{3}\,mL$

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