(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?

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Question 1: Kinetic Molecular Theory of Gases
(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?
Transcribed Image Text:Question 1: Kinetic Molecular Theory of Gases (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?
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