gases and unit test

Kinetic-Molecular Theory (KMT)

Explains the behavior of gases based on the motion of their particles.

Postulates of KMT

The assumptions that describe ideal gas behavior including constant motion, elastic collisions, negligible volume of gas particles, lack of intermolecular forces, and proportional average kinetic energy to temperature.

Elastic Collision

A collision where there is no net loss of kinetic energy.

Real Gas Behavior

Behavior of gases at high pressures and low temperatures where KMT assumptions break down due to significant intermolecular forces.

Gas Pressure

The force exerted per unit area due to gas particle collisions with container walls.

Boyle's Law

At constant temperature, the product of pressure and volume is constant (P1V1 = P2V2).

Viscosity

A measure of a fluid's resistance to flow.

Surface Tension

The strong intermolecular forces at a liquid's surface that affect how liquids behave.

Crystalline Solids

Solids with particles arranged in a periodic, repeating pattern exhibiting long-range order.

Amorphous Solids

Solids that lack long-range order; their atomic or molecular structure is disordered.

Endothermic Process

A phase change that requires energy input, such as boiling or melting.

Exothermic Process

A phase change that releases energy, such as condensation.

Intensive Property

A property that is independent of the amount of substance present (e.g., density, boiling point).

Extensive Property

A property that depends on the amount of substance present (e.g., mass, volume).

Chemical Property

Describes a substance's tendency to undergo chemical reactions and change its composition.

Physical Property

A property observable or measurable without changing the substance's composition.

Miscible Liquids

Liquids that can dissolve into one another.

Immiscible Liquids

Liquids that do not dissolve into one another.