Gas molecules move randomly, have elastic collisions, are point-like, and have no interactions {kinetic theory}|. Ideal gases follow kinetic theory. Gas molecules have cross-sectional area, and hydrogen bonds and van der Waals forces make molecules slightly attract, so real gas molecules do not move completely randomly and have somewhat inelastic collisions.
molecular collisions
In gases, one cubic centimeter has 10^28 molecular collisions per second. Collision frequency increases as mass decreases, temperature increases, cross-sectional area increases, and density increases.
molecular velocity
Gas-molecule collisions distribute speeds and directions. Molecular-velocity distributions are Boltzmann distributions. Some molecules have low velocity. Most molecules are near average velocity. Few molecules have very high velocities. Average gas-molecule velocity at room temperature is 500 meters per second. Molecular velocity increases as mass decreases or temperature increases.
Physical Sciences>Physics>Heat>Kinetics
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Date Modified: 2022.0224