[" The rate constant for a reaction at temperature "200K" is "10" time less than the rate "],[" constant at "400K" .What is the activation energy "(E_(a)" ) of the reaction."]

The rate constant of a reaction at temperature 200 K is 10 times less than the rate constant at 400 K. What is the activation energy (E_(a)) of the reaction ? (R = gas constant)

The rate constant of a reaction at temperature 200 K is 10 times less than the rate constant at 400 K. What is the activation energy (E_(a)) of the reaction ? (R = gas constant)

The rate constant of a reaction at 200K is 10 times less than rate constant at 400K. Value of E_a ? [R = gas constant]

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.

Write down the Arrhenius equation relating the rate constant of reaction with temperature , mentioning what the terms indicate. If k_(1) and k_(2) be the rate constant of a reaction at temperature t_(1)^(@)C and t_(2)^(@)C , respectively, find out the relation between k_(1) ,k_(2) and t_(1) and t_(2) . Given that the activation energy (E_(a)) of the reaction remains unchanged within the temperature range mentioned. The rate constant of a reaction at 400K and 500K are 0.02s^(-1) and 0.08s^(-1) respectively . Determine the activation energy (E_(a)) of the reaction.

The rate constant for first order reaction becomes six times when the temperature is raised from 50 K to 400 K. Calculate the activation energy for the reaction. (R= 8.314 J/K/mol)