The collisions of the particles with the walls of the container are the cause

The collisions of the particles with the walls of the

• Notes
• 35

This preview shows page 8 - 20 out of 35 pages.

Kinetic Molecular Theory
Kinetic Molecular Theory
Some move fast, some slow, speeds change Move in straight lines between collisions Path is random 5.6: Molecular Motion Collisions between gas particles and between particles and container walls are elastic collisions.
5.6: Molecular Motion ???𝑐𝑒 ? = 2?? ? 2 ? 𝑃 = ? 𝐴 𝑃𝑎??𝑖𝑐?𝑒 𝑃?𝑒????𝑒 = 2?? ? 2 ? + 2?? ? 2 ? + 2?? ? 2 ? 6? 2 𝑃𝑎??𝑖𝑐?𝑒 𝑃?𝑒????𝑒 = 2? ? ? ? 2 + ? ? 2 + ? ? 2 6? 2 = ?? 2 3? 3 𝐴?𝑔𝑒?𝑎𝑔𝑒 𝑃𝑎??𝑖𝑐?𝑒 𝑃?𝑒????𝑒 = ? ? 2 3? 3
5.6: Molecular Motion 𝐴?𝑔𝑒?𝑎𝑔𝑒 𝑃𝑎??𝑖𝑐?𝑒 𝑃?𝑒????𝑒 = ? ? 2 3? 3 𝑃 = ?𝑁 𝐴 ? ? 2 3𝑉 ?? 𝑎𝑣𝑔 = 𝑁 𝐴 1 2 ? ? 2 𝑃 = 2 3 ?𝑁 𝐴 1 2 ? ? 2 𝑉 𝑃 = 2 3 ?(??) 𝑎𝑣𝑔 𝑉 ?? 𝑃𝑉 ? = 2 3 (??) 𝑎𝑣𝑔
5.6: Molecular Motion 𝑃𝑉 ? = 2 3 (??) 𝑎𝑣𝑔 𝑃𝑉 ? = 𝑅𝑇 Theory Experiment (??) 𝑎𝑣𝑔 = 3 2 𝑅𝑇
One more relationship N A m= M, mass of a mole of gas particles in kilograms R = use the 8.3145 J K -1 mol -1 [joule (J) = kg m 2 s -2 ]
Distribution
Distribution Maxwell-Boltzmann distribution
Distribution Maxwell-Boltzmann distribution