PHYS-2210 Study Guide - Final Guide: Root Mean Square, Ideal Gas, Ideal Gas Law
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2 Apr 2016
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Kinetic theory attempts to model the random collisions of gas molecules on the walls of their container and relate it to the pressure (a macroscopic variable) they produce. What follows is a simplified version of kinetic theory used to relate pressure to the velocities of molecules in an ideal gas. Imagine a cube of length of side d full of ideal gas. The gas molecules are not stationary by have a random distribution of velocities. Some molecules move fast and others move slowly, and the directions of these velocities are also random. First we consider what happens to one molecule and then consider the combined effect of all n molecules. Image one of these molecules of mass m striking the wall of its container: Notice only the x-component of the velocity contributes to the force on the wall because the y and z components are parallel to the surface and don"t push on the wall.