Chapter 17 Vocabulary : Equilibrium

Introductory Chemistry

Collision model

Theory stating that reactants must collide with sufficient energy to react.

Activation energy (Ea)

The minimum energy that reacting species must possess to undergo a reaction.

Catalyst

A substance that speeds up a reaction without being consumed in the process.

Enzymes

Biological catalysts that increase the rate of chemical reactions in cells.

Equilibrium

A state where the concentrations of reactants and products remain constant.

Chemical equilibrium

The dynamic state where the rate of the forward reaction equals the reverse rate.

Law of chemical equilibrium

The relationship between the concentrations of reactants and products at equilibrium.

Equilibrium expression

A mathematical ratio of product concentrations to reactant concentrations at equilibrium.

Equilibrium constant (K)

A number that expresses the ratio of products to reactants at equilibrium.

Equilibrium position

The relative concentrations of reactants and products at equilibrium.

Homogeneous equilibria

Equilibria in which all reactants and products are in the same phase.

Heterogeneous equilibria

Equilibria involving reactants or products in different phases.

Le Châtelier’s principle

When a system at equilibrium is disturbed, it shifts to counteract the change.

Solubility product constant (Ksp)

The equilibrium constant for a saturated solution of a sparingly soluble salt.

Solubility product

Another term for the solubility product constant (Ksp).