CH5-3 (1).pdf - General Chemistry Chapter 5 Gases Lecture 3 of 3 $ Kinetic-Molecular Theory $ Root Mean Square Velocity $ Molecular Effusion and

CH5-3 (1).pdf - General Chemistry Chapter 5 Gases Lecture 3...

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1 General Chemistry Chapter 5: Gases Lecture 3 of 3 $ Kinetic-Molecular Theory $ Root Mean Square Velocity $ Molecular Effusion and Diffusion $ Real Gases: Deviations from Ideal Gas Behaviour Kinetic Molecular Theory (KMT) Up to this point we have been predicting how gases behave but not why they behave in the manner that they do. In order to explain the why of gases the Kinetic Molecular theory was developed. In summary the kinetic-molecular theory is: 1. The size of each gas particle is negligibly small. 2. The average kinetic energy of a particle is proportional to the temperature in kelvins. 3. The collision of one particle with another (or with the walls of its container) is completely elastic.
2 Questions from the gas simulator. True or False? S If you increase the pressure on a gas sample by decreasing the volume, the gas particles will speed up. S The pressure exerted by a gas depends on its molar mass. S The speed of a gas particle depends on its molar mass.

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