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 $V= \frac{nRT}{P}$
$=\frac{(0.10\,mol)(0.0821\,L\,atm\,mol^{-1}K^{-1})(300.\,K)}{0.9605\,atm}$
$=2.6\,L=2.6\times10^{3}\,mL$
