Properties of Gases and The Ideal Gas Law

These flashcards cover key vocabulary and concepts related to the properties of gases, the ideal gas law, and related principles, helping students understand and recall critical information for their exam.

Properties of Gases

Gases do not have definite volume or shape, have low densities, mix readily, and change volume with temperature.

Absolute Temperature

The temperature measured on the Kelvin scale, starting from absolute zero.

Boyle's Law

States that the pressure and volume of a gas are inversely proportional at constant temperature and moles (P1V1 = P2V2).

Charles's Law

States that the volume of a gas is directly proportional to its absolute temperature at constant pressure and moles (V1/T1 = V2/T2).

Avogadro’s Law

States that the volume of a gas is directly proportional to the number of moles of gas at constant temperature and pressure (V1/n1 = V2/n2).

Ideal Gas Law

The equation PV = nRT, used to relate pressure, volume, amount of gas in moles, and temperature.

Universal Gas Constant (R)

A constant used in the ideal gas law, with values such as 0.0821 L atm/(mol K) or 8.314 J/(mol K) depending on the units used.

Partial Pressure

The pressure contributed by a single gas in a mixture of gases.

Kinetic Molecular Theory

A model that describes gases as composed of small particles in random motion, with properties including negligible volume and elastic collisions.

Effusion

The process by which gas molecules escape through a tiny hole into a vacuum or lower pressure area.

Diffusion

The process by which molecules spread from areas of high concentration to areas of low concentration.