Pseudo Order Reaction Define
The reaction which appears to be higher order kinetic but actually follow lower order kinetic is called Pseudo order reaction.
We can understand the concept of pseudo order reaction with the help of following example :-
Ex : CH_3 COOC_2 H_5+H_2 O → CH_3 〖COOH+C〗_2 H_5 OH
Experimentally found that –
Rate =K[CH_3 COOC_2 H_5 ][H_2 O]
Rate =K^′ [CH_3 COOC_2 H_5]
Order of reaction =1
COLLISION THEORY OR CONCEPT OF ACTIVATION ENERGY
According to collision theory reactant molecules collide with each other to form product but all types of collision are not responsible for the formation of product only fraction of collision are responsible for the formation of product.
There are two types of collision on the basis of collision theory :-
(i)EFFECTIVE :- Such type of collision which are responsible the formation of product is called effective collision.
(ii)INEFFECTIVE :- Such type of collision which are not responsible for the formation of product is called ineffective collision.
- The minimum energy posesed by reactant molecules for effective collision is called threshold energy.
- It is denoted by E_T.
- The additional energy which must be observed by reactant molecules so that they achieve threshold energy or energy or energy barrier is called activation energy.
- It is denoted by E_a.
- The value of activation energy is always positive.
- Activation energy = Threshold energy-Enthalpy of reactant
E_P= Enthalpy of product
E_R= Enthalpy of reactant
E_T= Threshold energy
E_a= Activation energy of reactant.
E_a^′= Activation energy of product
vFor Exothermic –