1 / 4

Understanding Gas Behavior Through Kinetic Molecular Theory

Explore the foundations of the Kinetic Molecular Theory to understand why gases behave as described by the ideal gas equation. Discover how gas molecules in constant, random motion affect volume, interactions, and collisions. Learn about real gas deviations at low temperatures and high pressures, and how the Van der Waals equation corrects for them.

reed
Télécharger la présentation

Understanding Gas Behavior Through Kinetic Molecular Theory

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related