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Section6_KMT - Kinetic Molecular Theory of Gases By the end...

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Page 1 of 17 Kinetic Molecular Theory of Gases By the end of this lecture, you will be able to: (1) State the principles underlying the kinetic molecular theory of gases (2) Determine the average kinetic energy and the root mean square velocity of a gas particle (3) Understand effusion and state Graham ʼ s Law
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Page 2 of 17 Kinetic Molecular Theory of Gases This assumes that gases are made up of microscopic particles (atoms and/or molecules) that are in constant motion. The postulates of KMT are: (a) The particles are tiny compared to the distances between them, i.e. , the volume of the particles themselves is negligible compared to the volume of the container. (b) The particles exert no attractive or repulsive forces on one another.
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Page 3 of 17 (c) Collisions between particles are perfectly elastic ( i.e. , no energy loss in collision) and collisions of particles with the walls of the container are responsible for the observed pressure of the gas. (d) The average kinetic energy of the particles is directly proportional to the Kelvin temperature of the gas. The first two postulates are those identical to the requisites for ideality.
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Page 4 of 17 Some Mathematics Consider a particle of an ideal gas confined to a cube of length L . The particle has a velocity, u , which can be broken down into three spatial components, u x , u y , and u z .
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