Kinetic Molecular Theory

Based on the idea that particles of matter are always in motion

Ideal gas- hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory

1. Gases consist of large number of tiny particles that are far apart relative to their size

2. Collisions between gas particles and between particles and container walls are elastic collisions

elastic collision- one in which there is no net loss of total kinetic energy

3. Gas Particles are in continuous, rapid, random motion.

4. There are no forces of attraction between gas particles.

5. The temperature of a gas depends on the average kinetic energy of the particles of the gas.

Expansive- gases fill any container they are enclosed in and take its shape

Fluidity- gas particles slide easily past one another like a liquid

Low density- gases arre about 1/1000 the density of their liquid states.

Compressibility- a given sample of gas can be greatly decreased

Diffusion- spontaneous mixing of the particles of two substances caused by theri random motion

Effusion- a process by which gas particles pass through a tiny opening into a vacuum

a gas that does not behave completely according to the assumptions of the kinetic-molecular theory.

At high pressures and low temp., gas particles will be close, kinetic energy will not be able to overcome attractive forces. Going against ideal behavior

Noble gases show ideal behavior over many temps and many pressures

More polar molecules have greater attractive forces and therfore more likely to deviate from ideal behavior.