The mass action law and the Equilibrium constant

On the basis of observations of various equilibrium reactions, the two Norwegian chemists which were Goldberg and Waage suggested (in the year 1864) a quantitative relationship between the rates of reactions and the concentration of the reacting substances. This relationship is called as law of mass action. It can be stated as follows

The Rate of chemical is directly proportional to the product of the molar concentrations of reactants at the constant temperature at any given time.

The molar concentration that is the number of moles per liter is also known active mass. It is expressed by enclosing symbols of formulae of the substance in the square brackets. For instance, molar concentration of A is expressed as [A].

Consider the simple reversible reaction which is given as follows

          (At a certain temperature)

According to law of mass action

Rate of forward reaction 

Rate of backward reaction 

At equilibrium ,

The rate of forward reaction = The Rate of backward reaction

        Here,  is called as equilibrium constant.

In terms of partial pressures, equilibrium constant is denoted by K_p and

In terms of  mole fraction, equilibrium constant is denoted by K_x and

Relation between K_p, K_c and K_x

Dn = number of moles of gaseous products - number of moles of gaseous reactants in chemical equation.

As a rule, the concentration of pure solids and pure liquids are not included when writing an equilibrium equation.

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