The rate of a reaction at 200 K is 10 times less than the rate of the reaction at 400 K. Calculate activation energy of the reaction.

The rate of a reaction at 400 K is 10 times than the rate of the reaction at 200 K . Calculate activation energy of the reaction.

The rate of a reaction at 37^(@)C is twice the rate of the reaction at 27^(@)C . The activation energy (kJ.mol^(-1)) of the reaction is -

The rate of a reaction quadruples when the temperature changes from 293K to 313K. Calculate the energy of activation of the reaction assuming that it does not change with temperature.

The rate of a reaction increases four times when the temperature changes from 300 K to 320 K. Calculate the energy of activation of the reaction assuming that it does not change with temperature.

A hydrogenation reaction is carried out at 500K.If the same reaction is carried out in the presence of a catalyst at the same rate temperature required is 400K. Calculate the activation energy of the reaction if the catalyst lowers the activation barrier by 20"kJ.mol"^(-1)

The rate constant of a reaction at 200k is 0.1 times its value at TK . If the energy of activation of the reaction is 7.65"kJ.mol"^(-1) , find the value of 'T'?

Specific reaction rates for a reaction at 300K and 310K are 3xx10^(-6) S^(-1) and 2.8xx10^(-5 S^(-1 . Calculate the activation enrgy for that reaction.

The decomposition of H_(2)O_(2) is a first order reaction . The rate constant of the reaction can be expressed as logk=14.34-(1.25xx10^(4))/(T) . Calculate the activation energy of the reaction . At what temperature does the half-life of the reaction become 265min?

At 300K , frequency factor (A) of a first order reaction is 1000 times its rate constant . The activation energy of the reaction ("in kJ. Mol"^(-1)) is -

The rate constant of a first order reaction becomes 6 times when the temperature is raised from 350 K to 410K. Calculate the energy of activation for the reaction.