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