CHEM 112 Lecture Notes - Lecture 9: Kinetic Theory Of Gases, Rudolf Clausius, Ludwig Boltzmann
13 Oct 2014
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Kinetic molecular theory (kmt: to gain a better understanding of gases, Ludwig boltzmann developed the kinetic theory of gases. It can be used to predict properties of gases at low pressures and explain why real gases deviate from the ideal gas law. Kinetic molecular theory: particles are point masses (no volume) in constant, random, straight line motion, particles are separated by great distances, collisions are rapid and elastic, no force between particles, total energy remains constant. Forces (for 1 molecule: translational kinetic energy, (m=mass molecule, u=speed, frequency of collisions, (n = no. molecules) Impulse or momentum transfer: pressure (product of impulse and frequency) proportional to impulse times frequency e = k. Mean squared speed of all molecules (because they do not all have same speed) Average kinetic energy is directly proportional to temperature! (t) e k. Consider a single molecule moving in a cube of dimension l.
