Question

For carbon dioxide, the numerical value of ± is 3.592 and the numerical value of b is 0.0429.

Use the van der Waals equation to calculate the pressure of a sample of carbon dioxide at 85.0 °C with a molar volume of 4.89 L/mol.

Answer 1

Using the van der Waals equation, the pressure of the sample of carbon dioxide at 85.0 °C with a molar volume of 4.89 L/mol is approximately 0.963 atm.

To calculate the pressure of a sample of carbon dioxide at 85.0 °C with a molar volume of 4.89 L/mol, we can use the van der Waals equation:

P = (RT)/(V - b) - (a/v^2)

where P is the pressure, R is the ideal gas constant (0.0821 L·atm/(mol·K)), T is the temperature in Kelvin (85.0 + 273.15 = 358.15 K), V is the molar volume (4.89 L/mol), a is the attraction constant (± value = 3.592), b is the size constant (0.0429).

Substituting the given values into the equation:

P = (0.0821 * 358.15)/(4.89 - 0.0429) - (3.592/(4.89^2))

Calculating the expression:

P = 0.963 atm

Therefore, the pressure of the sample of carbon dioxide at 85.0 °C with a molar volume of 4.89 L/mol is approximately 0.963 atm.