Focus Guide for Exam IV CH 10 & 11

This set of flashcards covers key concepts related to the properties and behavior of gases as well as important laws and definitions relevant to chapters 10 and 11 in preparation for Exam IV.

Kinetic Molecular Theory (KMT)

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

Graham’s Law of Effusion

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

Ideal Gas Law

An equation of state for an ideal gas, represented as PV=nRT.

Dalton’s Law of Partial Pressure

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

Mole Fraction

A measure of the concentration of a component in a mixture, defined as the ratio of the moles of a component to the total moles of all components.

Exothermic Process

A process that releases heat to its surroundings.

Endothermic Process

A process that absorbs heat from its surroundings.

Intermolecular Forces

Forces that mediate interaction between molecules, including hydrogen bonding, dipole-dipole, and London Dispersion Forces.

Triple Point

The condition at which all three phases (solid, liquid, gas) of a substance coexist in thermodynamic equilibrium.

Phase Diagram

A graphical representation of the physical states of a substance under different conditions of temperature and pressure.