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

Volume $V=10.0\,L$ Number of moles $n=\frac{1.00\,g}{18.015\,g/mol}=0.0555\,mol$ Universal gas constant $R= 0.0821\,L\,atm\,mol^{-1}K^{-1}$ Temperature $T=(150.\,+273)K= 423\,K$ Recall that $PV=nRT$ (ideal gas law) $\implies$ Pressure $P= \frac{nRT}{V}$ $=\frac{(0.0555\,mol)(0.0821\,L\,atm\,mol^{-1}K^{-1})(423\,K)}{10.0\,L}$ $=0.193\,atm$