The rate of a reaction double when its temperature changes from 300K to 310K activation energy of such reaction will be (R=8.314`JK^(-1)mol^(-1)`)

The rate of a reaction doubles when its temperature changes from 300 K to 310 K . Activation energy of such a reaction will be: (R = 8.314 JK^(-1) mol^(-1) and log 2 = 0.301)

The rate of a reaction quadruples when the temperature changes from 300 to 310 K. The activation energy of this reaction is : ( Assume Activation energy and pre-exponential factor are independent of temperature, ln(2) = 0.693, R = 8.314J - mol^(-1) K^(-1))

The rate of a reaction becomes 4 times when temperature is raised from 293 K to 313 K. The activation energy for such reaction would be

The rate of a reaction triples when temperature changes from 50^@ C to 100^@ C. Calculate the energy of activation for such a reaction. ( R = 8.314 JK^(-1) mol^(-1) log 3 = 0.4771 )

The rate of reaction triples when temperature changes form 20^(@)C to 50^(@)C . Calculate the energy of activation for the reaction (R= 8.314JK^(-1)mol^(-1)) .

The rate constant for a first order reaction becomes six times when the temperature is raised from 350 K to 400 K. Calculate the activation energy for the reaction [R=8.314JK^(-1)mol^(-1)]

The rates of most reaction double when their temperature is raised from 298K to 308K . Calculate their activation energy.

Arrhenius studies the effect of temperature on the rate of a reaction and postulted that rate constant varies with temperature exponentially as k=Ae^(E_(a)//RT) . Thuis method is generally used for finding the activation energy of a reaction. Keeping temperature constant, the effect of catalyst on the activation energy has also been studied. If the rate of reaction doubles for 10^(@)C rise of temperature form 290K to 300K, the activation energy of the reaction will be approximately :