What Is Keq In Chemistry?

The equilibrium constant is calculated as the proportion of the product of the molar concentrations of the products to the products of the molar concentrations of the reactants, for each concentration term increased to the power of the stoichiometric coefficient in the regulated chemical reaction.

At a given temperature, the equilibrium constant is the proportion of the forward and reverse reaction rate constants.

The equilibrium constant of a chemical reaction (often indicated by the letter K) provides insight into the connection between products and reactants when a chemical reaction reaches equilibrium.

For instance, the equilibrium constant of concentration (indicated by Kc) of a chemical reaction at equilibrium is the ratio of the concentration of products to the concentration of reactants, each raised to their respective equilibrium data.

It is essential to recognize that multiple equilibrium constants give relationships between the products and reactants of equilibrium processes in terms of different units.

For a chemical reaction, the equilibrium constant is the ratio between the amount of reactant and the amount of product used to determine chemical behavior.

The forward reaction rate equals the reverse reaction rate at equilibrium.

i.e. rf = rb Or, kf × α × [A]a[B]b = kb × α × [C]c [D]d

The rate constants are constant at a certain temperature. The ratio between the rate constants of forwarding and reverse reactions should be constant and is known as the equilibrium constant (Kequ).

Equilibrium Constant – Characteristics

At a steady temperature, it is fixed and reaction-specific.
A catalyst alters the rates of both forward and reverses reactions in a manner that does not impact the equilibrium constant.
Changes in concentration, pressure, temperature and inert gases can influence equilibrium, favoring either forward or reverse reaction, but not the equilibrium constant.
G0 = -RT ln Kequ; this formula relates to the standard free energy.
Kequ has variable values at various temperatures for the same reversible reaction.
The equilibrium constant of the reverse equilibrium is the reciprocal of the initial equilibrium constant, or Krev = 1/Kequ.
Whenever the equilibrium reaction stoichiometry is altered, the equilibrium constant’s power is also altered by the same amount.
If the equilibrium constant for A + B C + D is K, then the equilibrium constant for 3A = 3B 3C + 3D is K3.
In the stepwise multiple equilibria leading to the final products, the equilibrium constant of the net equilibrium is equal to the product of the stepwise equilibrium constants. Consequently, the net equilibrium constant K equals K1 K2 K3.
Equilibrium reactions occur simultaneously with a shared product. The equilibrium constant does not vary for the reactions. The product concentrations will decrease due to the increased concentration of the common product.