Law of Mass action

  

Law of Mass action

In 1864, scientists Gulberg and Wage provided the law of mass action.

Law of Mass Action

 For a reversible reaction at equilibrium, the rate of a chemical reaction at constant temperature is proportional to the products of the concentrations of each reacting substance. 

A+B ------- Product

Rate α  [A] x [B]

Rate = K x [A] x [B]

That is, 

 A+B=CD

K₁[A]x[B]= K₂[C]x[D]

K₁/K₂=[C]x[D]/[A]x[B]

 K=[C]x[D]/[A]x[B]    {  K₁/K₂ = K}

K is the  rate constant

But if the reaction is like that,

3A + 2B ------ Product

However, according to the formula of mass, the mole numbers will become the power of the product.

A + 2B ------ Product

Rate α [A] x [B]

Rate = K x [A] ³ x [B]

But theoretically it is not always possible. Because Rate Low is the relationship between the density of the reactant and the rate of the reaction. This is only possible by the experimental results.

Such as:

2NO₂ (g) + F₂(g)= 2NO₂F(g)

This reaction was supposed to be as follows:

Rate=K  x  [NO₂]² +[F₂]

But the tested results do not happen. If we check, we will get

Rate=K  x   [NO₂] +[F₂]

(See in Bangla)