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

$1.07\times10^{3}\,L$
$n= 42.8\,mol$ (value from 26a) $P=600.\, mmHg\times\frac{1\,atm}{760\, mmHg}=0.7895\,atm$ $T= (-33+273)K= 240.\,K$ $R=0.0821\,L\,atm\,mol^{-1}K^{-1}$ $PV=nRT$ (ideal gas law) $\implies V=\frac{nRT}{P}=\frac{(42.8\,mol)(0.0821\,L\,atm\,mol^{-1}K^{-1})(240.\,K)}{0.7895\,atm}$ $=1.07\times10^{3}\,L$