What is the ratio of rate constants at 305 K and 300 K , if the activation energy of a reaction is 58.3 kJ/mol ?

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)

If the half-lives of the first order reaction at 350 K and 300 K are 2 and 20 seconds respectively, the activation energy of the reaction in kJ "mol"^(-1) is :

Rate of reaction at "400K" with " catalyst is equal to rate of reaction at "500K" without catalyst.What will be the activation energy of reaction if the catalyst lower the activation energy by "20KJ/mol

The rate constant is given by the Arrhenius equation as : k = Ae^(-Ea)//RT Calcualte the ratio of the catalysed and uncatalysed rate constants at 25^(@) C If the energy of activation of a analysed reaction is 162 kJ mol^(-1) and for uncatalysed reaction, the value is 350 kJ mol^(-1) .

A colliison between reactant molecules must occur with a certain minimum energy before it is effective in yielding Product molecules. This minimum energy is called activation energy E_(a) Large the value of activation energy, smaller the value of rate constant k . Larger is the value of activation energy, greater is the effect of temperature rise on rate constant k . E_(f) = Activation energy of forward reaction E_(b) = Activation energy of backward reaction Delta H = E_(f) - E_(b) E_(f) = threshold energy The activation eneries for forward and backward reactions in a chemical reaction are 30.5 and 45.4 kJ mol^(-1) respectively. The reaction is