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Kinetic Molecular Theory (KMT)

Describes the behavior of gas particles: they move in constant, random motion, collisions are elastic, and there are no attractions between particles.

Boyle's Law

States that P1V1 = P2V2 when temperature is held constant.

Charles's Law

States that V1/T1 = V2/T2 when pressure is held constant.

Ideal Gas Law

Describes the relationship between pressure, volume, temperature, and the number of moles of a gas: PV = nRT.

Graham's Law

Relates the rates of effusion of two gases to their molar masses: Rate1/Rate2 = (M2/M1)^(1/2).

Expansion (gas property)

Gases spread out to fill their container.

Diffusion

Random mixing of gases.

Real vs Ideal Gases

Ideal gases follow the KMT perfectly, while real gases have volume and intermolecular forces.

Surface tension

The inward pull at the surface of a liquid.

Triple point

The condition under which all three phases of a substance coexist.

Melting

The phase change from solid to liquid.

Vaporization

The phase change from liquid to gas.

Energy formula for phase changes

q = mΔH (for melting, freezing, boiling, condensation).

Phase diagram critical point

The end of the liquid-gas boundary, above which a supercritical fluid exists.

Compressibility (gas property)

Gases have high compressibility, making them easy to compress.

Kelvin to Celsius conversion

Kelvin = Celsius + 273.

STP conditions

Standard Temperature and Pressure: 0 °C = 273 K and 1 atm.