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14.0 moles of methane gas are in a 8.00- L tank at 20.5°C. Calculate the difference in pressure between methane and an ideal gas under these conditions. The van der Waals constants for methane are: a = 2.300 (L² atm/mol²) and b 0.0430 L/mol W Difference in pressure = atm (enter as positive number and use 3 sig figs)

14.0 moles of methane gas are in a 8.00- L tank at 20.5°C. Calculate the difference in pressure between methane and an ideal gas under these conditions. The van der Waals constants for methane are: a = 2.300 (L² atm/mol²) and b 0.0430 L/mol W Difference in pressure = atm (enter as positive number and use 3 sig figs)

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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14.0 moles of methane gas are in a 8.00- L tank at 20.5°C. Calculate the difference in pressure between methane and an ideal gas under these conditions. The van der Waals constants for methane are: a = 2.300 (L² atm / mol²) and b 0.0430 L/mol = Difference in pressure atm (enter as positive number and use 3 sig figs)
Transcribed Image Text:14.0 moles of methane gas are in a 8.00- L tank at 20.5°C. Calculate the difference in pressure between methane and an ideal gas under these conditions. The van der Waals constants for methane are: a = 2.300 (L² atm / mol²) and b 0.0430 L/mol = Difference in pressure atm (enter as positive number and use 3 sig figs)
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