(K, Keq) equilibrium constant expression; law of mass action. Compare with reaction quotient. The product of the concentrations of the products, divided by the product of the concentrations of the reactants, for a chemical reaction at equilibrium. For example, the equilibrium constant for A + B = C + D is equal to [C][D] / ([A][B]), where the square brackets indicate equilibrium concentrations. Each concentration is raised to a power equal to its stoichiometric coefficient in the expression. The equilibrium constant for A + 2B = 3C is equal to [C]3/([A][B]2). For gas phase reactions, partial pressures can be used in the equilibrium constant expression in place of concentrations.
the ratio of concentrations of products to reactants for a reaction at chemical equilibrium.
Ratio of forward and reverse rate constants for a reaction. For a binding reaction, A + B 1 2 AB, it equals the association constant, a; the higher the a, the tighter the binding between A and B. The reciprocal of the a is the dissociation constant, D; the higher the D, the weaker the binding between A and B.
a number representing the ratio of products to reactants in an equilibrium reaction
For any reversible reaction, the equilibrium constant is equal to the product of the concentrations of products divided by the product of the concentrations of reactants.
Value that describes the equilibrium state of the reversible reaction between two molecular species.
eq): the ratio of product concentrations to reactant concentrations with each raised to a power given by the number of moles of the substance in the balanced chemical equation of a reaction that has reached equilibrium; it indicates whether the reactants or products are favored in the reversible reaction.
Ratio of forward and reverse rate constants for a reaction and equal to the association constant.
An expression of chemical equilibrium under defined conditions. K is defined as the ratio of the forward and reverse rate constants for a chemical reaction. At equilibrium K equals the product of the reactant concentrations divided by the product of the r
(chemistry) the ratio of concentrations when equilibrium is reached in a reversible reaction (when the rate of the forward reaction equals the rate of the reverse reaction)
Value that expresses how far the reaction proceeds before reaching equilibrium. A small number means that the equilibrium is towards the reactants side while a large number means that the equilibrium is towards the products side.
The value (K eq) of the equilibrium constant expression for a system at equilibrium; a value greater than one indicates the position of equilibrium lies toward products, and a value less than one indicates the position of equilibrium lies toward reactants.
the value obtained when equilibrium concentrations of the chemical species are substituted into the equilibrium expression.
An expression involving the concentrations of reactants and products involved in a reaction. This expression yields a constant value regardless of the concentrations. The constant changes only with temperature.
The product of the concentrations (or activities) of the substances produced at equilibrium in a chemical reaction divided by the product of concentrations of the reacting substances, each concentration raised to that power which is the coefficient of the substance in the chemical equation.
A quantity that characterizes the position of equilibrium for a reversible reaction; its magnitude is equal to the mass action expression at equilibrium. K varies with temperature.
according to the law of mass action, for any reversible chemical reaction: aA + bB = cC + dD, the equilibrium constant ()is defined as: = ([C]c[D]d)/([A]a[B]b)
In chemistry, the equilibrium constant is a quantity characterizing a chemical equilibrium in a chemical reaction. It is a useful tool in determining the concentration of various reactants and products in a system where chemical equilibrium occurs.