Lecture 11 - Lecture 11 Special Topics on Gases Kinetic...

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Lecture 11: Special Topics on Gases Kinetic Theory of Gases—Assumptions Hard, spherical particles in constant random motion Velocity (speed and direction, the vector v) is constant until a collision occurs Most of the volume is empty space There are no forces on the particles, including from other particles or the walls of the container holding the gas All collisions are elastic; energy is transferred among particles, but is not lost The temperature is a measure of the average kinetic energy (the book states it the opposite way). Kinetic energy = ½(mv 2 ). Note that for heavier particles, v 2 is proportionally lower than for lighter particles at the same temperature. Restatement of ideal gas law: PV = (1/3)(nM v rms 2 ), derived on pages 160-163. M = mass of one mole of molecules v rms = (3RT/M) 1/2 which relates temperature to kinetic energy and velocity Kinetic Theory of Gases—consequences If n changes, P changes proportionally. The more particles, the more collisions
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This note was uploaded on 09/29/2009 for the course ME 530.230 taught by Professor Katz during the Spring '09 term at Johns Hopkins.

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Lecture 11 - Lecture 11 Special Topics on Gases Kinetic...

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