Gas Laws and Kinetic Molecular Theory

Flashcards covering key concepts related to gas laws and kinetic molecular theory.

Kinetic Molecular Theory

A theory that states particles of gas are in constant motion and collide with one another and the walls of their container.

Boyle's Law

States that the pressure and volume of a gas are inversely proportional at constant temperature and moles (P1xV1 = P2xV2).

Charles's Law

Describes the direct proportionality between the temperature and volume of a gas at constant pressure and moles (V1/T1 = V2/T2).

Avogadro's Law

Indicates the relationship between temperature and pressure of a gas at constant moles and volume, stating that they are directly proportional (P1/T1 = P2/T2).

Ideal Gas

A hypothetical gas composed of particles that are in constant motion and exhibit perfectly elastic collisions and negligible volume.

Ideal Gas Law

The equation that describes the state of an ideal gas, represented as PV = NRT, where R is a constant equal to 0.08206.

Dalton's Law of Partial Pressure

States that the total pressure of a gas sample is the sum of the partial pressures of its individual components.

Mole Fraction

The ratio of the amount of one component in a mixture to the total amount of all components, calculated as mole of gas/total moles.

Graham's Law of Effusion

States that the rate of effusion of a gas is inversely proportional to the square root of its molar mass (R2/R1 = square root(MOLAR MASS1/MOLAR MASS2)).