# Problem: Calculate the pressure that CCl4 will exert at 41 oC if 1.20 mol occupies 33.6 L , assuming thatCCl4 obeys the van der Waals equation. (Values for the van der Waals constants are a=20.4, b=0.1383.)

###### FREE Expert Solution

We’re being asked to calculate the pressure exerted by a CCl4 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 (Latm)/(molK)
T = temperature, K
a = polarity coefficient
= size coefficient

Let’s first isolate the pressure in the Van der Waals Equation:

91% (181 ratings) ###### Problem Details

Calculate the pressure that CCl4 will exert at 41 oC if 1.20 mol occupies 33.6 L , assuming that

CCl4 obeys the van der Waals equation. (Values for the van der Waals constants are a=20.4, b=0.1383.)