Rate law the Molecularity and Order of a reaction  

The Molecularity is sum of the number of molecules of reactants involved in the balanced chemical equation. The Molecularity of a whole reaction has no importance and overall kinetics of the reaction depends upon the rate determining step. The slowest step is rate-determining step. This was given by Van't Hoff.

Example :

Total number of the molecules or atoms whose concentration determines the rate of reaction is called as order of reaction.

The Order of reaction = Sum of the exponents of the concentration terms in rate law

For the reaction xA+yB→Products

The rate law is Rate = [A]^x[B]^y

Then the overall order of the reaction. n=x+y

Here x and y are orders with respect to the individual reactants.

         · If the reaction is in form of reaction mechanism then the order is determined by slowest step of mechanism.

         (Here, the overall order of the reaction is equal to two.)

         · The Molecularity of a reaction is derived from mechanism of the given reaction. The Molecularity cannot be greater than three because more than three molecules might not mutually collide with each other.

         · The Molecularity of a reaction can't be zero, negative or fractional. Order of the reaction can be zero, negative, positive or in fraction and greater than three. The Infinite and imaginary values are not possible.

         · It one of the reactants is present in the excess, the second order reaction conforms to the first order and is called as pesudo unimolecular reaction. 

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