What is the pressure of 1.00 mole of #Cl_2# gas that is non-ideal, at a temperature of 0.0 deg C occupying a volume 34.6 L?
The pressure is 0.652 bar.
I assume that you are treating the chlorine as a van der Waals gas.
The van der Waals equation is
#color(blue)(bar(ul(|color(white)(a/a) (P + (n^2a)/V^2)(V - nb) = nRTcolor(white)(a/a)|)))" "#
#P + (n^2a)/V^2 = (nRT)/(V - nb)#
#P = (nRT)/(V - nb)- (n^2a)/V^2#
For this problem,
The pressure predicted by the van der Waals equation is 0.652 bar.
Note: The Ideal Gas Law predicts a pressure of 0.656 bar. Under these conditions, chlorine is behaving almost like an ideal gas.