Gas Laws and Kinetic-Molecular Theory

These flashcards cover key terms and concepts related to gas laws and kinetic-molecular theory, providing foundational definitions for exam preparation.

Absolute Zero

The lowest possible temperature (0 K) where molecular motion stops.

Ideal Gas Law

PV = nRT; describes the physical behavior of an ideal gas using pressure, volume, temperature, and amount.

Molar Mass

The mass of a given substance (chemical element or chemical compound) divided by the amount of substance.

Density of an Ideal Gas

Density is defined as (molar mass)P/RT, and can vary with changes in temperature and pressure.

Dalton’s Law of Partial Pressures

In a mixture of ideal gases, the total pressure is equal to the sum of the partial pressures of individual gases.

Kinetic-Molecular Theory of Gases

A theory that explains the behavior of gases based on the idea that gas is made of a large number of small particles in constant, random motion.

Effusion

The escape of gas molecules through a tiny hole into a vacuum.

Diffusion

The spread of particles as a result of random thermal motion.

Universal Gas Constant (R)

A constant used in the ideal gas law, typically 0.08206 (L·atm)/(mol·K).

Molecular Speed

The speed of a gas particle, which increases with temperature, affecting the kinetic energy.

Mean Free Path

The average distance a molecule travels between collisions.