Chapter 9 Gases- the Simplest State of Matter

These flashcards cover key vocabulary and concepts related to the properties and laws governing gases, as outlined in Chapter 9 of the lecture notes.

Kinetic Molecular Theory of Gases

A theory that describes the behavior of gases in terms of particles in motion.

Pressure

The force applied per unit surface area, caused by the collisions of gas molecules with the walls of a container.

Boyle's Law

A gas law stating that the volume of a gas is inversely proportional to its pressure at constant temperature.

Charles's Law

A gas law that describes the direct proportionality of gas volume to its temperature at constant pressure.

Avogadro’s Law

A gas law stating that the volume of a gas is directly proportional to the number of moles of gas at constant temperature and pressure.

Mean Free Path

The average distance a gas molecule travels before colliding with another molecule.

Ideal Gas Law

An equation of state for an ideal gas that relates pressure, volume, number of moles, and temperature (PV=nRT).

Dalton’s Law of Partial Pressures

A law stating that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases.

Diffusion

The process of gradual mixing of molecules of one gas with another due to their kinetic properties.

Effusion

The process by which a gas escapes through a small opening.

Real gas behavior

Behavior of gases that deviates from ideal gas laws, typically at high pressures and low temperatures.

Van der Waals equation

An equation that modifies the ideal gas law to account for molecular size and intermolecular forces.