Van der Waals Equation Video Lessons

Concept

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

###### FREE Expert Solution

We are asked why the pressure of Ne is higher than that predicted for an ideal gas based on van der Waals 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:

88% (479 ratings)
###### Problem Details

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