Kinetic Molecular Theory

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Slide 1

Kinetic Molecular Theory

ki⋅net⋅ic

Origin: 1850–55; < Gk kīnētikós moving, equiv. to kīnē- (verbid s. of kīneîn to move) + -tikos

Source: Websters Dictionary

Slide 2

CA Standards

Slide 3

The Nature of Gases

Gases expand to fill their containers

Gases are fluid – they flow

Gases have low density

1/1000 the density of the equivalent liquid or solid

Gases are compressible

Gases effuse and diffuse

Slide 4

Kinetic Molecular Theory

Particles of matter are ALWAYS in motion

Volume of individual particles is  zero.

Collisions of particles with container walls cause the pressure exerted by gas.

Particles exert no forces on each other.

Average kinetic energy is proportional to Kelvin temperature of a gas.

Slide 5

Kinetic Energy of Gas Particles

At the same conditions of temperature, all gases have the same average kinetic energy.

m = mass

v = velocity

 At the same temperature, small molecules move FASTER than large molecules

Slide 6

Diffusion

Diffusion describes the mixing of gases. The rate of diffusion is the rate of gas mixing.

Diffusion is the result of random movement of gas molecules

The rate of diffusion increases with temperature

Small molecules diffuse faster than large molecules

Slide 7

Graham’s Law of Diffusion

M1 = Molar Mass of gas 1

M2 = Molar Mass of gas 2

Slide 8

Purification of Uranium-235 Using Gaseous Diffusion