Use the van der Waal's equation to calculate the pressure (in atm) exerted by 1.00 mol of chlorine gas confined to a volume of 2.00 L at 273K. The value of a = 6.49 L2 atm mol-2, and that of b = 0.0562 L mol-1 for chlorine gas.
a) no given answer is close
We’re being asked to calculate the pressure exerted by a chlorine gas using the Van der Waal’s equation.
The Van der Waals equation is shown below:
▪ P = pressure, atm
▪ V = volume, L
▪ n = # of moles, mol
▪ R = gas constant = 0.08206 (L∙atm)/(mol∙K)
▪ T = temperature, K
▪ a = polarity coefficient
▪ b = size coefficient
Let’s first isolate the pressure in the Van der Waals Equation: