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According to the ideal gas law, a 0.9244 mol sample of oxygen gas in a 1.983 L container at 268.1 K should exert a pressure of 10.26 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For O2 gas, a = 1.360 L²atm/mol? and b = 3.183×10-2 L/mol. |Pideal – Pvan der Waals - Percent difference x 100 Pideal +Pvan der Waals 2

According to the ideal gas law, a 0.9244 mol sample of oxygen gas in a 1.983 L container at 268.1 K should exert a pressure of 10.26 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For O2 gas, a = 1.360 L²atm/mol? and b = 3.183×10-2 L/mol. |Pideal – Pvan der Waals - Percent difference x 100 Pideal +Pvan der Waals 2

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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According to the ideal gas law, a 0.9244 mol sample of oxygen gas in a 1.983 L container at 268.1 K should exert a pressure of 10.26 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For O2 gas, a = 1.360 L²atm/mol? and b = 3.183×10-2 L/mol. |Pideal – Pvan der Waals Percent difference x 100 Pideol+Pvan der Waals 2 According to the ideal gas law, a 9.629 mol sample of nitrogen gas in a 0.8290 L container at 496.3 K should exert a pressure of 473.0 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For N2 gas, a = 1.390 L²atm/mol? and b = 3.910×10-2 %3D L/mol. |Pideal - Pvan der Waals Percent difference = х 100 Pideal+Pvan der Waals 43.6 % An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.
Transcribed Image Text:According to the ideal gas law, a 0.9244 mol sample of oxygen gas in a 1.983 L container at 268.1 K should exert a pressure of 10.26 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For O2 gas, a = 1.360 L²atm/mol? and b = 3.183×10-2 L/mol. |Pideal – Pvan der Waals Percent difference x 100 Pideol+Pvan der Waals 2 According to the ideal gas law, a 9.629 mol sample of nitrogen gas in a 0.8290 L container at 496.3 K should exert a pressure of 473.0 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For N2 gas, a = 1.390 L²atm/mol? and b = 3.910×10-2 %3D L/mol. |Pideal - Pvan der Waals Percent difference = х 100 Pideal+Pvan der Waals 43.6 % An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.
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