The ratio of rate constants of a reaction at 300K and 291K is 2. Calculate the energy of activation. `("Given "R = "8.314JK"^(-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) ].

(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 equilibrium constant for the reaction is 10. Calculate the value of DeltaG^(@) , Given R=8.314JK^(-1)"mol"^(-1)T=300K

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))

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) ]

The rate constant of a reaction is doubled when the temperature increased from 400K to 410K. Calculate the activation energy (Ea) [R = 8.314 JK^(-1) " mol"^(-1)] .

A plot of (1)/(T) Vsk for a reaction gives the slope - 1 xx 10^(4)K . The energy of activation for the reaction is (Given R = 8.314 JK^(-1) " mol"^(-1) )