Water vapor is a polar gas molecule. Because of this it has fairly strong interactions with itself in the gas phase that can make it behave less like an ideal gas that other gases under similar conditions. What is the difference between the calculated pressures found using the ideal gas law and found using the van der Waals gas equation for 1 mole of water vapor at -100°C in a 1.00 L container. (van der Waals constants for water are a = 5.464 L2 atm mol-2, b = 0.03049 Lmol-1) i atm

Water vapor is a polar gas molecule. Because of this it has fairly strong interactions with itself in the gas phase that can make it behave less like an ideal gas that other gases under similar conditions. What is the difference between the calculated pressures found using the ideal gas law and found using the van der Waals gas equation for 1 mole of water vapor at -100°C in a 1.00 L container. (van der Waals constants for water are a = 5.464 L2 atm mol-2, b = 0.03049 Lmol-1) i atm

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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