According to the ideal gas law, a 1.075 mol sample of xenon gas in a 1.270 L container at 270.1 K should exert a pressure of 18.76 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Xe gas, a = 4.194 L2atm/mol2 and b= 5.105x102 L/mol. |Pideal - Pvan der Waals Percent difference = x 100 Pdeal+Pean der Waals 2
According to the ideal gas law, a 1.075 mol sample of xenon gas in a 1.270 L container at 270.1 K should exert a pressure of 18.76 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Xe gas, a = 4.194 L2atm/mol2 and b= 5.105x102 L/mol. |Pideal - Pvan der Waals Percent difference = x 100 Pdeal+Pean der Waals 2
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter10: Gases And Their Properties
Section: Chapter Questions
Problem 53PS: In the text, it is stated that the pressure of 4.00 mol of Cl2 in a 4.00-L tank at 100.0 C should be...
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