Calculate the ratio of the catalysed and uncatalysed rate constant at `20^(@)C` if the energy of activation of a catalysed reaction is `20 kJ "mol"^(-1)` and for the uncatalysed reaction is `75 kJ "mol"^(-1)`

The rate constant is given by the Arrhenius equation as : k = Ae^(-Ea)//RT Calcualte the ratio of the catalysed and uncatalysed rate constants at 25^(@) C If the energy of activation of a analysed reaction is 162 kJ mol^(-1) and for uncatalysed reaction, the value is 350 kJ mol^(-1) .

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

Calculate the log_(10) of the ratio of the catalysed and uncatalysed rate constant at 25^(@) C. If at this temperature the energy of activation of a catalysed reaction is 162KJ and for the uncatalysed reaction the value is 350 KJ (Assume frequency factor is same for both reaction)

The rate of catalysed reaction is large than the uncatalysed reaction as ___

A 1st order reaction is 50% complete in 30 minute at 27^(@)C and in 10 minute at 47^(@)C . Calculate the: (a) Rate constant for reaction at 27^(@)C and 47^(@)C . (b) Energy of activation for the reaction. (c ) Energy of activation for the reverse reaction if heat of reaction is -50 kJ mol^(-1) .

For A+B rarr C+D, DeltaH=-20 kJ mol^(-1) , the activation energy of the forward reaction is 85 kJ mol^(-1) . The activation energy for backward reaction is …… kJ mol^(-1) .