Kinetic-Molecular Theory

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Presentation transcript:

Kinetic-Molecular Theory All particles are in constant motion. Explains properties of matter.

Ideal Gas = follows K-M theory 5 Assumptions 1. Lots of tiny particles that are far apart 2. Elastic collisions = no loss of energy 3. Have kinetic energy (KE) – constant motion 4. No forces of attraction or repulsion between particles 5. Average KE depends on temp.

Expansion No definite shape or volume Gases ‘expand’ to fit any ‘container’

Fluidity Density Gas particles easily flow past each other. Very low Particles are very far apart.

Compressibility Particles pushed together Decreases volume

Diffusion Effusion Mixing of particles caused by random motion Ex: perfume can be smelled across the room Effusion Gas particles pass through tiny openings Ex: Helium balloon slowly ‘deflates’

Temperature Measure of the energy (movement) of particles Units of Temperature Degrees Celsius (C) Kelvin (K) ºCelsius + 273 = Kelvin Lord Kelvin

Pressure (P) Force per unit area

Units of Pressure Millimeters of Mercury (mm of Hg) Torrs Atmospheres (atm) kiloPascals (kPa) Pounds per square inch (psi)

Measuring Pressure Barometer Measures atmospheric pressure Height of mercury depends on atmospheric pressure

Manometer Measures an enclosed gas.