Question

As an ideal gas, 1 mol of carbon dioxide would occupy 22.4 L at 273 K at 1 atm pressure. Use the van der Waals equation to predict the actual pressure of 1 mol of carbon dioxide in a volume of 22.4 L at 273 K. For carbon dioxide, a = 3.59 L2 atm mol-2 and b = 0.0427 L mol-1.

A. 0.990 atm
B. 0.995 atm
C. 1.000 atm
D. 1.005 atm
E. 1.010 atm

Answer 1

To predict the actual pressure of 1 mol of carbon dioxide in a volume of 22.4 L at 273 K using the van der Waals equation, the actual pressure is approximately 1.010 atm.

Step-by-step explanation:

To predict the actual pressure of 1 mol of carbon dioxide in a volume of 22.4 L at 273 K using the van der Waals equation, we can use the formula:

(P + a(n/V)^2)(V - nb) = nRT

Where P is the pressure, a and b are constants specific to the gas, n is the number of moles, V is the volume, R is the ideal gas constant, and T is the temperature. For carbon dioxide, a = 3.59 L^2 atm mol^-2 and b = 0.0427 L mol^-1.

Substituting the given values into the equation:

(P + 3.59(1/22.4)^2)(22.4 - 0.0427) = (1)(0.0821)(273)

Simplifying and solving for P, the actual pressure of 1 mol of carbon dioxide in the given volume at 273 K is approximately 1.010 atm.