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Kinetic Molecular Theory

Kinetic Molecular Theory. WHY do gases behave the way the ideal gas equation says they do? . Gases consist of a large # of molecules that are in constant, random motion The volume of the molecules is negligible compared to the total volume of the gas

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Kinetic Molecular Theory

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  1. Kinetic Molecular Theory WHY do gases behave the way the ideal gas equation says they do?

  2. Gases consist of a large # of molecules that are in constant, random motion • The volume of the molecules is negligible compared to the total volume of the gas • Gas molecules do not attract or repel each other • Collisions are perfectly elastic – energy is not transferred between molecules during collisions • The average kinetic energy is proportional to the temperature of the system

  3. Real Gas Deviations • Low temperature and High pressure Deviate because – 1. Gas molecules do have volume 2. Gas molecules do attract/repel

  4. Van der Walls equation • Corrects for real gases P + n2a V – nb = nRT V2

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