(a) A 4.25-L flask contains 3.46 mol CO2 at 229 °C. The pressure of this gas calculated from the ideal gas law is 33.5 atm. From the van der Waals equation the pressure is 32.4 atm. i. Give an (adequate) reason(s) for the difference. ii. What is the compression factor for this gas at the real temperature and pressure? ii.Under which of the following sets of conditions is a real gas expected to deviate from ideal behaviour?
(a) A 4.25-L flask contains 3.46 mol CO2 at 229 °C. The pressure of this gas calculated from the ideal gas law is 33.5 atm. From the van der Waals equation the pressure is 32.4 atm. i. Give an (adequate) reason(s) for the difference. ii. What is the compression factor for this gas at the real temperature and pressure? ii.Under which of the following sets of conditions is a real gas expected to deviate from ideal behaviour?
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 40PS: A collapsed balloon is filled with He to a volume of 12.5 L at a pressure of 1.00 atm. Oxygen, O2,...
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