Equilibrium constant
Equilibrium Constant (K_eq)
The Equilibrium Constant (/ˈiːkwɪˈlɪbriəm ˈkɒnstənt/), also known as K_eq, is a measure of the ratio of the concentrations of products to reactants at equilibrium in a chemical reaction. The concept of the equilibrium constant was first introduced in the late 19th century by the French chemist Le Chatelier and the German chemist Haber.
Etymology
The term "Equilibrium Constant" is derived from the Latin word "aequilibrium" meaning balance, and the Latin word "constans" meaning standing together. It refers to the state of balance in a chemical reaction where the rate of forward reaction equals the rate of the reverse reaction.
Definition
In a general chemical reaction represented as:
aA + bB ⇌ cC + dD
The equilibrium constant (K_eq) is given by:
K_eq = ([C]^c [D]^d) / ([A]^a [B]^b)
where [A], [B], [C], and [D] represent the molar concentrations of the reactants and products, and a, b, c, and d are their respective stoichiometric coefficients.
Types of Equilibrium Constants
There are several types of equilibrium constants, including the acid dissociation constant (K_a), the base dissociation constant (K_b), the solubility product constant (K_sp), and the formation constant (K_f).
Related Terms
External links
- Medical encyclopedia article on Equilibrium constant
- Wikipedia's article - Equilibrium constant
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