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 :

The rate constants for a reaction at 400 K and 500 K are 2 . 60 xx 10^(-5) s^(-1) and 2.60 xx 10^(-3) s^(-1) respectively. The activation energy of the reaction in kJ mol^(-1) is

The half life of a first order reaction is 900 min at 820 K.Estimate its half life at 720 K if the energy of activation of the reaction is 250 kJ mol^(-1)

At 300K , frequency factor (A) of a first order reaction is 1000 times its rate constant . The activation energy of the reaction ("in kJ. Mol"^(-1)) is -

A reaction occurs in three steps . The rate constants of the first , second and third steps of the reaction are k_(1), k_(2) and k_(3) respectively and the overall rate constant of the reaction is k=k_(1)k_(2)//k_(3) . If the activation energies of the first , second and third step of the reaction are 30, 44 and 56"kJ.mol"^(-1) respectively , then the overall activation energy of the reaction ("in kJ.mol") is -

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 is lowered to 50 kJ "mol"^(-1) at the same teperature. How many times the rate of reaction will change ?

A first order reaction is 50% complete in 25 minutes at 350 K. Calculate activation energy of the reaction.

The activation energy of a first order reaction at 300 K is kJ mol^(-1) . In the presence of a catalyst, the activation energy gets lowered to 50kJ mol^(-1) at 300 K . How many times the reaction rate change in the presence of a catalyst at the same temperature ?

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 50kJ mol^(-1) at 300 K . How many times the reaction rate change in the presence of a catalyst at the same temperature ?