According to the ideal gas law, a 10.24 mol sample of xenon gas in a 0.8381 L container at 499.4 K should exert a pressure of 500.7 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 5.105×102 L/mol. Percent difference = |Pideal - Pvan der Waals x 100 Pideal + Pvan der Waals % 2

According to the ideal gas law, a 10.24 mol sample of xenon gas in a 0.8381 L container at 499.4 K should exert a pressure of 500.7 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 5.105×102 L/mol. Percent difference = |Pideal - Pvan der Waals x 100 Pideal + Pvan der Waals % 2

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

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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You have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted with a piston. The density of this mixture at STP is 1.924 g/L. Assume ideal behavior and constant temperature and pressure. a. What is the mole fraction of He in the original mixture? b. The SO2 and O2 react to completion to form SO3. What is the density of the gas mixture after the reaction is complete?
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 26.0 atm if calculated using the van der Waals equation. Verify this result, and compare it with the pressure predicted by the ideal gas law.
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