Chapter 5: Gases and the Kinetic-Molecular Theory

Flashcards covering key concepts related to gases and the Kinetic-Molecular Theory for exam preparation.

Gas

A state of matter where molecules are far apart, move freely, and fill the available space.

Liquid

A state of matter where molecules are close together but can move around one another.

Solid

A state of matter where molecules are close together in a regular array and do not move around one another.

Gas Pressure

The force exerted by gas molecules colliding with the walls of their container.

Standard Temperature and Pressure (STP)

Standard conditions defined as 0 °C (273.15 K) and 1 atm (101.325 kPa).

Boyle's Law

Describes the inverse relationship between the volume of a gas and its pressure when temperature and the amount of gas are held constant.

Charles's Law

Describes the direct relationship between the volume of a gas and its Kelvin temperature when pressure and the amount of gas are held constant.

Avogadro's Law

States that the volume of a gas is proportional to the number of moles present when temperature and pressure are held constant.

Ideal Gas Law

The equation PV = nRT which relates pressure (P), volume (V), amount of substance (n), and temperature (T) of an ideal gas.

Kinetic Molecular Theory

A model that explains the behavior of gases in terms of particle movement and collisions.

Dalton's Law of Partial Pressures

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

Effusion

The process by which a gas escapes through a small hole into a vacuum.

Diffusion

The mixing of gas molecules due to their random motion.

Graham's Law

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