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:

$\overline{)\left(\mathbf{P}\mathbf{+}\mathbf{a}\frac{{\mathbf{n}}^{\mathbf{2}}}{{\mathbf{V}}^{\mathbf{2}}}\right)\left(\mathbf{V}\mathbf{-}\mathbf{n}\mathbf{b}\right){\mathbf{=}}{\mathbf{n}}{\mathbf{R}}{\mathbf{T}}}$

▪ **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**:

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 L^{2} atm mol^{-2}, and that of b = 0.0562 L mol^{-1 }for chlorine gas.

a) no given answer is close

b) 9.9

c) 4.12

d) 1.54

e) 3.73

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