Ideal Gas Law and Kinetic Theory Overview

Ideal Gas Law

Relates pressure, volume, temperature, and moles.

Avogadro's Number

Number of particles in one mole, approximately 6.022 x 10²³.

Mole

Amount of substance containing Avogadro's number of particles.

Molecular Mass

Mass of a molecule, measured in atomic mass units (u).

Atomic Mass Unit (u)

Unit for measuring atomic and molecular masses.

Boyle's Law

At constant temperature, pressure inversely proportional to volume.

Charles' Law

At constant pressure, volume directly proportional to temperature.

Kinetic Theory

Describes gas behavior based on particle motion and collisions.

Elastic Collisions

Collisions where total kinetic energy is conserved.

Root-Mean-Square Speed

Average speed of gas molecules, calculated from kinetic energy.

Pressure

Force exerted per unit area by gas molecules.

Temperature (Kelvin)

Absolute temperature scale used in gas law calculations.

Volume

Space occupied by gas, inversely related to pressure.

Internal Energy

Total energy contained within a system, related to temperature.

Alveoli

Tiny air sacs in lungs where gas exchange occurs.

Oxygen Concentration

Percentage of oxygen in air, approximately 14% in alveoli.

Gas Constant (R)

Constant used in ideal gas law equations, 8.314 J/(mol·K).

Density

Mass per unit volume of a substance.

Macroscopic Level

Observations made on a large scale, not molecular.

Nitrogen Molecule

N₂, molecular mass of 28.0 u.

Oxygen Molecule

O₂, molecular mass of 32.0 u.

Gas Behavior

Describes how gases respond to changes in conditions.