Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Transcribed Image Text:8:21 >4OB 00 •
83% i
00
Use the van der Waals equation of state to calculate the pressure of 4.00 mol of SO, at 453K in a 3.80 L vessel. Van der Waals
constants can be found in the van der Waals constants table.
Use the ideal gas equation to cakulate the pressure under the same conditions.
P =
39.15
atm
In a 16.80 L vessel, the pressure of 4.00 mol of SO, at 453 K is 8.85 atm when calculated using the ideal gas equation and
8.59 atm when calculated using the van der Waals equation of state.
II
Transcribed Image Text:8:22 >10 000 •
83% i
00
In a 16.80 L vessel, the pressure of 4.00 mol of SO, at 453 K is 8.85 atm when calkulated using the ideal gas equation and
8.59 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
3.80 L vessel compared to the 16.80L vessel?
O The attractive forces between molecules become less ofa factor at the hisher pressure in the 3,80L vessel.
O The molecular volume is a smaller part of the total volume of the 3.8OL vessel.
O The molecular volume is a larger part of the total volume of the 3.80L vessel.
O The attractive forces between molecules become a greater factor at the higher pressure in the 3.80 L vessel.
II
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