Chapter 5 - Gases_Part6 - GENERAL CHEMISTRY CHAPTER 5 GASES...

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GENERAL CHEMISTRY CHAPTER 5 – GASES PAGE 21 OF 23 b n P nRT V + = Ideal vs. Real Gases Real gases often do not behave like ideal gases at high pressure or low temperature Ideal Gas Laws assume: No attractions between gas molecules Gas molecules do not take up space based on the Kinetic Molecular Theory At low temperatures and high pressures these assumptions are not valid High Pressures The volume of a real gas is larger than predicted by the ideal gas law at high pressures The amount of space occupied by the molecules is a significant amount of the total volume The molecular volume makes the real volume larger than the ideal gas law would predict van der Waals modified the ideal gas equation to account for the molecular volume b = van der Waals constant and is different for every gas because their molecules are different sizes Because real molecules take up space, the molar volume of a real gas is larger than predicted by the ideal gas law at high pressures
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This note was uploaded on 01/21/2011 for the course PHYS 4A 60865 taught by Professor L. oldewurtel during the Fall '09 term at Irvine Valley College.

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Chapter 5 - Gases_Part6 - GENERAL CHEMISTRY CHAPTER 5 GASES...

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