Key Concepts in Gas Laws and Kinetic Theory

Kinetic Molecular Theory (KMT)

A theory that explains the behavior of gases by stating that all matter is made of particles in constant motion.

Compressibility

The ability of gases to be compressed due to the large spaces between particles.

Diffusion

The spreading of gas particles from high concentration to low concentration.

Effusion

The process by which gas particles pass through a tiny opening from one container to another.

Fluidity

The ability of gas particles to flow past one another, similar to liquids.

Molar Mass

The mass of one mole of a substance, typically measured in grams per mole (g/mol).

Pressure

The force that gas particles exert when they collide with the walls of their container.

Volume

The amount of space a gas occupies.

Temperature

A measure of the average kinetic energy of the gas particles, measured in Kelvin (K) for gas law calculations.

Amount (n)

The quantity of gas, usually measured in moles (mol).

Ideal Gas

A hypothetical gas that follows all gas laws perfectly, with no intermolecular forces or particle volume.

Real Gas

A gas that deviates from ideal behavior due to intermolecular forces and finite particle volume, especially under high pressure and low temperature.

Standard Temperature and Pressure (STP)

STP refers to a temperature of 0°C (273K) and a pressure of 1 atm (101.3 kPa).

Gas Constant (R)

A constant used in the Ideal Gas Law, with values typically 0.0821 L·atm/mol·K or 8.31 L·kPa/mol·K.

Boyle's Law

The inverse relationship between pressure and volume of a gas at constant temperature and moles.

Charles's Law

The direct relationship between volume and temperature of a gas at constant pressure and moles.

Gay-Lussac's Law

The direct relationship between pressure and temperature of a gas at constant volume and moles.

Combined Gas Law

A combination of Boyle's, Charles's, and Gay-Lussac's laws that describes the relationship between pressure, volume, and temperature when moles are constant.

Ideal Gas Law

An equation that describes the behavior of an ideal gas: PV=nRT.

Graham's Law

The relationship between the rates of diffusion or effusion of two gases and their molar masses.

Standard Pressure

1 atmosphere (atm), 101.3 kPa, or 760 mmHg.