The activation energy of a first order reaction at 300 K is 60 kJ `mol^-1`. In the Presence of a Catalyst, the activation energy gets lowered to 50 kJ `mol^-1` at 300 K. How many times the reaction rate changes in the Presence of a catalyst at the same temperature ?

At 27^@C in the presence of a catalyst, the activation energy of a reaction is lowered by 10 kJ mol^-1 . The ratio of log k (catalyst)/k (uncatalysed) is

The activation energy for the reaction 2 HI(g) rarr H_2 + I_2 (g) is 209.5 kJ mol^(-1) at 58IK.Calculate the fraction of molecules of reactants having energy equal to or greater than activation energy?

Activation energy for the acid catalysed hydrolysis of sucrose is 6.22 kJ mol^-1 , while the activation energy is only 2.15 kJ mol^-1 when hydrolysis is catalysed by the enzyme sucrase. Explain.

A hydrogenation reaction is carried out at 500 K . If the same reaction is carried out in the presence of a catalyst at the same rate, the temperature required is 400 K . Calculate the activation energy of the reaction if the catalyst lowers the activation barrier by 20 kJ mol^(-1) . a) 100 kJ/mol b) 80 kJ/mol c) 60 kJ/mol d) none of these

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: a) 40 Kcal mol^(-1) b) 12 Kcal mol^(-1) c) 60 Kcal mol^(-1) d) 70 Kcal mol^(-1)

For a first order reaction, k = 2.5xx10^-4 s^-1 , what is the rate of reaction, when the initial concentration of the reactant is 0.1 mol L^-1 ?

The activation energy of a reaction is 56.2 kJ/mol. The ratio of the rate constant at 300 K and 305 K is (R = 8 J "mole"^(-1)K^(-1) ) about :