Gas Laws and Kinetic Molecular Theory

These flashcards cover the key vocabulary and concepts from the Gas Laws and Kinetic Molecular Theory lecture, focusing on definitions and relationships essential for understanding gas behavior.

Kinetic Molecular Theory (KMT)

A model explaining the behavior of gases at the microscopic level through the motion and properties of gas particles.

Ideal Gas

A hypothetical gas whose molecules occupy negligible space and have no interactions, used to simplify gas laws.

Boyle’s Law

States that the volume of a gas varies inversely with pressure when temperature and number of moles are held constant.

Charles’s Law

States that the volume of a gas is directly related to its absolute temperature when pressure and number of moles are constant.

Gay-Lussac’s Law

States that the pressure of a gas is directly related to its absolute temperature when volume and number of moles are constant.

Avogadro’s Law

States that equal volumes of gases at the same temperature and pressure contain the same number of moles.

Dalton’s Law of Partial Pressures

States that the total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas.

Standard Temperature and Pressure (STP)

Defined as 0°C (273 K) and 1 atm pressure; used as a reference point for gas calculations.

Molar Volume

The volume occupied by one mole of a gas at standard temperature and pressure, which is 22.4 liters.

Gas Diffusion

The process by which gas molecules spread out through space and mix with other gases due to their random motion.