Calculate the pressure in atm that CCl4 exerts at 80 °C if 2.00 mol occupies 66.6 L, assuming that a) CCl4 obeys the ideal gas equation. b) CCl4 obeys the van der Waals equation. The van der Waals constant for CCl4 are a = 20.4 L2atm/mol2and b = 0.1383 L/mol.
Calculate the pressure in atm that CCl4 exerts at 80 °C if 2.00 mol occupies 66.6 L, assuming that a) CCl4 obeys the ideal gas equation. b) CCl4 obeys the van der Waals equation. The van der Waals constant for CCl4 are a = 20.4 L2atm/mol2and b = 0.1383 L/mol.
Introductory Chemistry: An Active Learning Approach
6th Edition
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Mark S. Cracolice, Ed Peters
Chapter4: Introduction To Gases
Section: Chapter Questions
Problem 51E
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Calculate the pressure in atm that CCl4 exerts at 80 °C if 2.00 mol occupies 66.6 L, assuming that
a) CCl4 obeys the ideal gas equation.
b) CCl4 obeys the van der Waals equation. The van der Waals constant for CCl4 are a = 20.4 L2atm/mol2and b = 0.1383 L/mol.
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