CHEM 102 Lecture Notes - Lecture 1: Van Der Waals Equation, Ideal Gas Law, Kinetic Theory Of Gases
14 Jan 2017
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Document Summary
Molecules in a gas don"t really interact (collisions considered elastic) because the molecules are so far apart that it is unlikely for an interaction to occur. This is false at low temperatures because at lower velocities it is more difficult to overcome attractive intermolecular forces ( sticky molecules) Liquid imfs must be considered in predictions/calculations. Greatest deviation from ideal gas law happens at low temperature and high pressure. Imfs reduce pressure (fewer collisions=fewer forces per unit area (pressure)) Volume of molecules are a significant fraction of total volume at high overall pressure and low overall volume because molecules are so close together. At low temperatures, the energy of the molecules can"t overcome the interaction of imfs. Real gas molecules hit the walls of the container with less force because of the imfs between the molecule and its neighboring. (cid:1853)/2=adjusts p for the molecular attraction (pressure is increased)
