Homogeneous equilibrium

Definition

Homogeneous equilibrium occurs when all reactants and products of a chemical reaction are in the same phase, usually liquid or gas. It is characterized by a constant ratio of the concentrations of reactants and products at equilibrium.

5 Must Know Facts For Your Next Test

1. In homogeneous equilibria, the equilibrium constant expression includes only species in the same phase.
2. The value of the equilibrium constant, $K$, remains unchanged with concentration changes but can be affected by temperature.
3. For gaseous reactions, the equilibrium constant can also be expressed in terms of partial pressures ($K_p$).
4. A homogeneous equilibrium can be described using either $K_c$ (concentration) or $K_p$ (partial pressure), depending on whether the species are in molarity or pressure units.
5. The presence of a catalyst does not affect the position of homogeneous equilibrium; it only speeds up reaching the equilibrium.

Review Questions

Related terms

Equilibrium Constant ($K$): $K$ quantifies the ratio of concentrations of products to reactants at equilibrium for a given reaction.

$K_c$: $K_c$ is the equilibrium constant expressed in terms of molar concentrations.

$K_p$: $K_p$ is the equilibrium constant expressed in terms of partial pressures for gaseous systems.