01:160:161 Lecture Notes - Lecture 32: Molar Mass, Jmol, Chemistry (Band)
21 Nov 2017
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Lecture #32 kinetic molecular theory: langowski. Mathematical relationships found in gas laws can be conceptually explained by the kinetic molecular theory. Temperature - measure of the average kinetic energy of a system or particle. Although different gases at the same temperature have the same average kinetic energy, they do not have the same velocities. Example: he (g) vs ne (g) at 373 k. He moves much faster than the neon atom. In a gas mixture at a given temperature, lighter particles move faster (on average) than heavier particles. K = mv2 this relationship explains why he moves faster than ne (it has a lighter mass, therefore its kinetic energy is greater) Conceptually and numerically similar to the average velocity. Under a given set of conditions, gas particles will exhibit a distribution of velocities. Heavier gases move slower than lighter gases. At a given temperature, lighter particles have a higher average velocity (and a broader distribution) than heavier particles.
