Question

Use the van der Waals equation of state to calculate the pressure of 2.10 mol of Kr at 471 K in a 3.70L vessel. Van der Waals constants can be found in this table. Number P- 2.004 atm Use the ideal gas equation to calculate the pressure under the same conditions. Number P= 21.947 atm In a 15.5 L vessel, the pressure of 2.10 mol of Kr at 471 K is 5.24 atm when calculated using the ideal gas equation and 5.15 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 3.70 L vessel compared to the 15.5 L vessel? The molecular volume is a larger part of the total volume of the 3.70 L vessel. The attractive forces between molecules become a greater factor at the higher pressure in the 3.70 L vessel. The attractive forces between molecules become less of a factor at the higher pressure in the 3.70 L vessel. The molecular volume is a smaller part of the total volume of the 3.70 L vessel.

Answer 1