Unit 3: Gases, States of Matter, & IMFS

This set of flashcards covers key concepts and terminologies related to gases, their behaviors, and intermolecular forces as outlined in the lecture notes.

Eponymous Gas Laws

The gas laws named after scientists that describe the relationships between gas variables.

Kinetic Molecular Theory (KMT)

A theory that explains the behavior of gases in terms of particles in motion and their energy.

Dalton's Law of Partial Pressures

The total pressure of a mixture of gases equals the sum of the individual partial pressures of each gas.

Ideal Gas Law

A relationship among pressure (P), volume (V), number of moles (n), and temperature (T) represented by the equation PV=nRT.

Graham's Law

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

Boyle's Law

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

Charles' Law

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

Avogadro's Law

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

Van der Waals Equation

An equation that accounts for the non-ideal behavior of gases by including correction factors for pressure and volume.

Intermolecular Forces

Forces of attraction between molecules, which include dispersion forces, dipole-dipole interactions, and hydrogen bonding.

Physical Properties of Liquids

Characteristics that can be directly related to intermolecular forces, such as viscosity and surface tension.

Combustion Reaction

A rapid reaction that produces heat and light, typically involving oxygen as a reactant.