Rate constant of reaction at 300 K and 400 K are `0.0345 S^(-1)` and `0.1365 S^(-1)` respectively. Calculate the activation energy for the reaction.
[Given : `R = 8.314 J K^(-1) mol^(-1)`]

The rate constant of a raction at 500 K and 700 K are 0.02 s^(-1) and 0.07s^(-1) respectively. Calculate the value of E_(a)

The rate constant of a first order reaction at 300 K and 310 K are respectively 1.2 xx 10^(3) s^(-1) and 2.4 xx 10^(3) s^(-1) . Calculate the energy of activation. (R = 8.314 J K^(-1) mol^(-1))

Show that R=8.314 Jmol^(-1)K^(-1)

(a) Derive an integrated rate equation for the rate constant of a first order reaction. (b) The specific reaction rate of a reaction quadruples when temperature changes from 30^(0) to 50^(0) .Calculate the energy of activation of the reaction. [Given : R = 8.314 JK^(-1)mol^(-1)] .

The specific reaction rate of a reaction quadruples when temperature changes from 30°C to 50°C. Calculate the energy of activation of the reaction [Given : R = 8.314 "JK"^(-1) "mol"^(-1) ]

a) The rate of a particular reaction doubles when the temperature changes from 300 K to 310 K. Calculate the energy of activation of the reaction. [Given : R="8.314 JK"^(-1)" mol"^(-1) ].