1 General ChemistryChapter 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 howgases behave but not whythey behave in the manner that they do. In order to explain the whyof gases the Kinetic Molecular theorywas 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? SIf you increase the pressure on a gas sample by decreasing the volume, the gas particles will speed up. SThe pressure exerted by a gas depends on its molar mass. SThe speed of a gas particle depends on its molar mass.