Gas Laws and Kinetic Molecular Theory

This set of flashcards covers key vocabulary and concepts related to gas laws and the behavior of gases as described by kinetic molecular theory.

Density (d)

Mass per unit volume, often expressed in g/L for gases.

Ideal Gas Law

PV = nRT, relates pressure, volume, temperature, and amount of gas.

Combined Gas Law

P1V1/T1 = P2V2/T2, relates pressure, volume, and temperature when the amount of gas is constant.

Gay-Lussac's Law

For a given sample of gas at constant volume, pressure is directly proportional to absolute temperature (K).

Charles' Law

For a given sample of gas at constant pressure, volume is directly proportional to absolute temperature (K).

Boyle's Law

For a given sample of gas at constant temperature, pressure is inversely related to volume.

Avogadro's Law

Equal volumes of gases at the same temperature and pressure contain the same number of particles.

Kinetic Molecular Theory (KMT)

A theory that describes the behavior of gases in terms of particles in motion.

Diffusion

The spreading of gas molecules from an area of higher concentration to lower concentration.

Effusion

The process by which gas particles pass through a tiny opening.

Absolute Zero

The theoretical temperature (0 Kelvin) at which all particle motion ceases.

Real Gas

A gas that does not behave ideally and has measurable volume and intermolecular forces.

Ideal Gas

A hypothetical gas whose particles have no volume and do not exert forces on each other.

Dalton's Law of Partial Pressures

In a mixture of gases, the total pressure is equal to the sum of the partial pressures of individual gases.

Pressure (P)

The force exerted by gas particles colliding with the walls of the container.

Volume (V)

The space occupied by a gas.

Temperature (T)

A measure of the average kinetic energy of gas particles.

Moles (n)

A measure of the amount of substance; can relate to the number of gas particles.