Rate constant for a chemical reaction taking place at 500K is expressed as `K=A. e^(-1000)` The activation energy of the reaction is :

Rate constant for a chemical reaction taking place at 500 K is expressed as k=A*e^(-1000) . The activation energy of the reaction is yxx 10^(6)"cal mol"^(-1) . y is ______. [R=2"cal mol"^(-1)K^(-1)]

The rate constant of a chemical reaction at 600K is 1.6xx10^(-5)s^(-1) . The activation energy of the reaction is 209"kJ.mol"^(-1) . Calculate its rate constant at 700K.

For a reaction, the rate constant is expressed as k = Ae^(-40000//T) . The energy of the activation is

For a reaction, the rate constant is expressed as k = Ae^(-40000//T) . The energy of the activation is

The rate constant of a chemical reaction at 280K is 1.6 xx 10^-6 s^-1 . The activation energy of this reaction is zero. The value of k for this reaction at 300K is

The temperature dependence on rate constant (k) of a chemical reaction is written in terms of Arrhenius equation, k=A.e^(-E^(0)//RT) . Activation energy (E^(0)) of the reaction can be calculated by plotting