Consider the following Vander Waals equation:

(P+ n²a/V²)(V-nb)=nRT

a. Explain the significance of the factors a and b in the equation

For CO₂ (g) a= 3.592 L²-atom/mol² and b=0.04267 L/mol

Assuming that at normal condition 1 mol of CO₂ at 0 C occupies a volume od 22.4 L

b. Using the ideal gas and Vander Waals equations, compute respectively the pressures of CO₂ .

Let's now repeat this calculation, assuming that the gas is compressed so that it fills a container that has a volume of only 0.200 liters.

c. Compute the pressures of CO₂ by using the ideal gas equation and Vander Waals equation.

d. What can be concluded from a and b