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.
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In homogeneous equilibria, the equilibrium constant expression includes only species in the same phase.
The value of the equilibrium constant, $K$, remains unchanged with concentration changes but can be affected by temperature.
For gaseous reactions, the equilibrium constant can also be expressed in terms of partial pressures ($K_p$).
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.
The presence of a catalyst does not affect the position of homogeneous equilibrium; it only speeds up reaching the equilibrium.
Review Questions
What distinguishes a homogeneous equilibrium from a heterogeneous one?
How does changing temperature affect the value of an equilibrium constant for a homogeneous reaction?
Can you write an expression for $K_p$ given a balanced chemical equation involving gases?
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.