Chemistry 2AChemistry 2A-c F2006 c F2006 (Ch6(Ch6-12)8312)83V. Simple Kinetic Molecular Model of Gases1. Molecules move randomly (in straight-line) until hitting the wall of the container.2. Volume of molecules are negligible: point-mass approximation. 3. Molecule-wall collisions are elastic (no loss in kinetic energy).4. No attractive forces between molecule-molecule & molecule-wall.5. The average kinetic energy of gaseous molecules is proportional to the temp. (in K). (To be derived later)Kinetic energy: KE =(1/2)mu2The average kinetic energy (<KE>): <KE> =(1/2)m<u2> (per molecule) = (1/2)M<u2> (per mol)Here M is the molecular weight, <u2> is the average of u2, and u is the velocity of the gaseous molecules
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