Chemistry equilibrium

Equilibrium

A state in which the forward and reverse reactions occur at equal rates in a reversible chemical reaction.

Dynamic Equilibrium

A condition where the rates of the forward and reverse reactions are equal, resulting in no net change in concentration of reactants and products.

Non-reversible Reactions

Reactions represented by a single arrow, indicating they do not reach equilibrium.

Reversible Reactions

Reactions represented by a double-headed arrow, indicating they can reach equilibrium.

Reactants

Substances that undergo a chemical change in a reaction.

Products

Substances that are formed as a result of a chemical reaction.

Equilibrium Law

A principle stating that at a given temperature, the ratio of the concentration of products to reactants is a constant.

Equilibrium Constant (Kc)

The constant value representing the ratio of concentrations of products to reactants at equilibrium, which varies with temperature.

Large Kc Value

Indicates that products are favored over reactants (Kc > 1).

Small Kc Value

Indicates that reactants are favored over products (Kc < 1).

Pure Solids and Liquids

Substances that are not included in the calculation of the Kc value.

Homogeneous Equilibrium

An equilibrium where reactants and products are in the same phase, commonly in the gaseous phase.

Heterogeneous Equilibrium

An equilibrium where reactants and products exist in different phases.

Kc of Reverse Reaction

The relationship that Kc (reverse) = 1/Kc (forward).

Effect of Pressure on Equilibrium

Increasing pressure favors the side of the reaction with fewer moles of gas.

Effect of Temperature on Equilibrium

In exothermic reactions, increasing temperature shifts equilibrium to the left, favoring reactants.

Catalyst

A substance that lowers activation energy and increases the rates of both forward and reverse reactions without changing Kc.

Le Châtelier Principle

A principle stating that if a change is made to a system at equilibrium, the system will adjust to counteract the change and restore equilibrium.

Reaction Quotient (Q)

A measure used to determine the progress of a reaction toward equilibrium when the system has not yet reached equilibrium.