Van der Waals Equation Video Lessons

Concept

# Problem: Assuming that the van der Waals equation predictions are accurate, account for why the pressure of He is higher than that predicted for an ideal gas.

###### FREE Expert Solution

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 (Latm)/(molK)
T = temperature, K
a = polarity coefficient
= size coefficient

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

###### Problem Details

Assuming that the van der Waals equation predictions are accurate, account for why the pressure of He is higher than that predicted for an ideal gas.