## General Chemistry: Principles and Modern Applications (10th Edition)

$n=13.7 \,g\,Cl_{2}\times\frac{1\,mol\,Cl_{2}}{70.906\,g\,Cl_{2}}=0.1932\,mol$ $R=0.08314\,bar\,L\,mol^{-1}K^{-1}$ $P=0.993\,bar$ $V=7.50\,L$ From the ideal gas law, we have $T=\frac{PV}{nR}=\frac{0.993\,bar\times7.50\,L}{0.1932\,mol\times0.08314\,bar\,L\,mol^{-1}K^{-1}}$ $=464\,K$