As an ideal gas, 1 mol of carbon dioxide would occupy 22.4 L at 273 K and 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/mol² and b = 0.0427 L/mol.

Question

Quizplus · Accepted Answer

To use the van der Waals equation, we need to convert the given temperature to Kelvin:
T = 273 K
Then, we can substitute the given values for a, b, n (number of moles), V (volume), R (gas constant), and T into the equation:
[P + (n^2a/V^2)](V - nb) = nRT
Solving for P, we get:
P = [nRT/(V - nb)] - n^2a/(V^2)
Substituting the given values, we get:
P = [(1 mol)(0.0821 L*atm/mol*K)(273 K)/(22.4 L - (1 mol)(0.0427 L/mol))] - (1 mol)^2(3.59 L*atm/mol^2)/(22.4 L)^2
P = 0.995 atm
Therefore, the best choice is B, which is the closest value to our calculation.

As an Ideal Gas, 1 Mol of Carbon Dioxide Would