#$1.($a$)$ Calculate the molar volume of chlorine gas at $350K$ and $2\mathrm{.}30$atm using the ideal gas law.

$($b$)$ Repeat part $($a$),$ but use the van der Waals equation of state. The van der Waals constants are $a=6\mathrm{.}493L^2$ atm $mo{l}^{-}2,$ and $b=0\mathrm{.}05622Lmo{l}^{-1}.$

Hint: try an iterative procedure, starting with the ideal gas volume as a first estimate for the attractive term. Do two iterations to reach the answer$)$