For a reaction, the rate constant is expressed as `k = Ae^(-40000//T)`. The energy of the activation is

Rate constant for a chemical reaction taking place at 500K is expressed as K=A. e^(-1000) The activation energy of the reaction is :

Rate constant for a chemical reaction taking place at 500K is expressed as K=A. e^(-1000) The activation energy of the reaction is :

Rate constant for a chemical reaction taking place at 500K is expressed as K=A. e^(-1000) The activation energy of the reaction is :

for a given reaction at temeperature T, the velocity constant k, is expressed as : k=ae^(-27000K'//T) (K' = Boltzmann constant) Given , R=2 cal K^(-1) "mol"^(-1) . Calculate the value of energy of activation. Comment on the results.

For a reaction AtoB with activation energy E_(a) and rate constant k=Ae^(-Ea//RT) . The rate of the reaction (Rate =k[A] ) increases by increasing the temperature because

A reaction takes place in three rate determining steps having rate constants K_(1), K_(2), K_(3) respectively. The overall rate constant K=(K_(1)K_(3))/K_(2) . If energy of activations for the three steps are respectively 10, 20, 40 kJ . The overall energy of activation is:

The rate constant is given by Arrhenius equation. k=Ae^(-E_(a)//RT) Calculate the ratio of the catalysed and uncatalysed rate constants at 25^(@)C if the energy of activation of a catalysed raction is 162 kJ and for the uncatalysed reaction the value is 350 kJ