Question

Use the van der Waals equation of state to calculate the pressure of 2.30 mol of N, at 483K in a 4.20 L vessel. Van der Waals constants can be found in the van der Waals constants table. P= atm Use the ideal gas equation to calculate the pressure under the same conditions. P= atm In a 16.10 L vessel, the pressure of 2.30 mol of N20 at 483 K is 5.66 atm when calculated using the ideal gas equation and 5.62 atm when calculated using the van der Waals equation of state. Why is the percent difference in the pressures calculated using the two different equations greater when the gas is in the 4.20 L vessel compared to the 16.10 L vessel? The molecular volume is a smaller part of the total volume of the 4.20L vessel. The molecular volume is a larger part of the total volume of the 4.20 L vessel. The attractive forces between molecules become less of a factor at the higher pressure in the 4.20L vessel. The attractive forces between molecules become a greater factor at the higher pressure in the 4.20 L vessel.

Answer 1

The percent difference in pressures calculated using the van der Waals equation and ideal gas equation is greater in the 4.20 L vessel compared to the 16.10 L vessel due to the smaller molecular volume of the gas.

Step-by-step explanation:

The percent difference in the pressures calculated using the two different equations is greater when the gas is in the 4.20 L vessel compared to the 16.10 L vessel because the molecular volume is a smaller part of the total volume in the 4.20 L vessel. The van der Waals equation of state takes into account the molecular volume and attractive forces between molecules, which become a greater factor at higher pressure and smaller volume. Therefore, when the volume is smaller, these molecular interactions have a bigger impact on the overall pressure calculation.