Chemistry: Kinetic Molecular Theory and Gas Properties

These flashcards cover key concepts from the lecture on the Kinetic Molecular Theory and properties of gases, helping students review essential terms and definitions.

Kinetic Molecular Theory (KMT)

A theory that describes the behavior of gases in terms of particles in constant motion, with negligible volume and interactions between them.

Diffusion

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

Effusion

The process of gas escaping through a tiny hole into a vacuum.

Elastic Collisions

Collisions between gas molecules where there is no net loss of kinetic energy.

Root Mean Square Speed (Urms)

The square root of the average of the squares of the speeds of the gas particles, used to calculate average speed.

Molar Volume

The volume occupied by one mole of an ideal gas at standard temperature and pressure (STP), approximately 22.7 liters.

Ideal Gas Law

A mathematical relationship between pressure, volume, temperature, and number of moles of a gas, expressed as PV=nRT.

Boyle's Law

The principle that the pressure of a gas is inversely proportional to its volume at a constant temperature.

Amonton's Law (Gay-Lussac's Law)

The law stating that the pressure of a gas is directly proportional to its absolute temperature when the volume is constant.

Combined Gas Law

A law that combines Boyle's, Charles', and Gay-Lussac's Laws to describe the relationship between pressure, volume, and temperature of a gas.

Density of Gas

The mass per unit volume of a gas, often expressed in grams per liter.

Standard Temperature and Pressure (STP)

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

Molar Mass (MM)

The mass of one mole of a substance, usually expressed in grams per mole.

Dalton's Law of Partial Pressures

A law stating that the total pressure exerted by a gas mixture is equal to the sum of the partial pressures of each individual gas.

Graham's Law of Effusion

A principle stating that the rate of effusion of a gas is inversely proportional to the square root of its molar mass.

Mean Free Path

The average distance a molecule travels between collisions with other molecules.

Absolute Temperature (T)

A temperature measured on the Kelvin scale, where absolute zero is 0 K.

Gauge Pressure

The pressure of a system measured relative to atmospheric pressure.

Compressibility

The ability of a gas to decrease in volume under pressure.

Miscibility of Gases

The ability of two or more gases to mix evenly in all proportions.