Equilibrium constant

Equilibrium Constant is a fundamental concept in the field of Chemistry, specifically in the study of Chemical Equilibrium. It is a measure of the ratio of the concentrations of products to reactants at equilibrium, with each concentration raised to the power of its stoichiometric coefficient in the balanced chemical equation.

Definition[edit | edit source]

The Equilibrium Constant (symbol: K) is defined for a general chemical reaction:

aA + bB ⇌ cC + dD

The equilibrium constant expression is given by:

K = ([C]^c [D]^d) / ([A]^a [B]^b)

where [A], [B], [C], and [D] represent the molar concentrations of the chemicals A, B, C, and D respectively, at equilibrium. The coefficients a, b, c, and d are the stoichiometric coefficients of the balanced chemical equation.

Types of Equilibrium Constants[edit | edit source]

There are several types of equilibrium constants, each used for different types of reactions:

Kc - used for reactions in which concentrations are expressed in molarity.
Kp - used for reactions involving gases, where concentrations are expressed in terms of partial pressures.
Ka and Kb - used for acid-base reactions.
Kw - the ion product of water.
Ksp - the solubility product constant.

Factors Affecting the Equilibrium Constant[edit | edit source]

The value of the equilibrium constant is temperature dependent. Changes in pressure, concentration, or the addition of a catalyst do not affect the value of the equilibrium constant, although they do affect the position of the equilibrium.

References[edit | edit source]

Equilibrium constant Resources
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