Equilibrium constant is useful in:
The magnitude of equilibrium constant provides a useful indication of the extent of a chemical reaction. The equilibrium constant for a reversible reaction is equal to the ratio of concentrations of product and the concentrations of the reactants.
A + B ⇌ C + D
Kc or Kp =
The magnitude of equilibrium constant Kc and Kp indicates the extent to which a reaction will proceed.
If the value of Kp>103, then the reaction proceeds to completion.
If the value of Kp <10-3 then the reaction proceeds rarely.
If the value of Kpis between10-3 to 103, then appreciable quantities of the reactants as well as the products are present.
At any point in a reversible reaction, the ratio of the concentration of the products to that of the reactants is known as the reaction quotient Q (Qc with molar concentrations and Qp with partial pressures).
Qc =
Qc =
The reaction quotient expression of a reaction has the same equation as the equilibrium constant expression for that reaction. Reaction quotient is calculated using the concentrations or pressure at a given point of time in the reaction, and not its equilibrium concentrations or pressures.
If Qc > Kc, backward reaction takes place.
If Qc < Kc, forward reaction takes place.
If Qc = Kc, the reaction is already at equilibrium.
Equilibrium constant is useful in:
The magnitude of equilibrium constant provides a useful indication of the extent of a chemical reaction. The equilibrium constant for a reversible reaction is equal to the ratio of concentrations of product and the concentrations of the reactants.
A + B ⇌ C + D
Kc or Kp =
The magnitude of equilibrium constant Kc and Kp indicates the extent to which a reaction will proceed.
If the value of Kp>103, then the reaction proceeds to completion.
If the value of Kp <10-3 then the reaction proceeds rarely.
If the value of Kpis between10-3 to 103, then appreciable quantities of the reactants as well as the products are present.
At any point in a reversible reaction, the ratio of the concentration of the products to that of the reactants is known as the reaction quotient Q (Qc with molar concentrations and Qp with partial pressures).
Qc =
Qc =
The reaction quotient expression of a reaction has the same equation as the equilibrium constant expression for that reaction. Reaction quotient is calculated using the concentrations or pressure at a given point of time in the reaction, and not its equilibrium concentrations or pressures.
If Qc > Kc, backward reaction takes place.
If Qc < Kc, forward reaction takes place.
If Qc = Kc, the reaction is already at equilibrium.