For a first order reaction K = `6.3 xx 10^(-18)``e^(-2600/T)` then the value of activation energy in KJ is

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 rate constant for a first order decomposition reaction is given by log K=10 - 1000/T .Then,what will be activation energy in kcal/mol?

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 ?

The energy of activation of a first order reaction is 187.06 kJ mol^(-1) at 750 K and the value of pre-exponential factor A is 1.97xx10^(12)s^(-1) . Calculate the rate constant and half life. (e^(-30)= 9.35xx10^(-14))

The substance undergoes first order decomposition.The decomposition follows two parallel first order reactons as : K_1=10^(-2) sec^(-1) and K_2=10^(-2)sec^(-1) If the corresponding activation energies of parallel reaction are 100 and 120 kJ "mol"^(-1) then the net activation energy of A is/are:

The rate constant for a second order reaction is given by k=(5 times 10^11)e^(-29000k//T) . The value of E_a will be:

The slope of Arrhenius plot (l_(n)k " vs " 1//J) of a first order reaction is -5 xx 10^(3) . The value of E_(a) of the reaction is (R = 8.314 J K^(-1)mol^(-1))

On introducing a ctatlyst at 500 K, the rate of a first order reaction increases by 1.718 times. The activation energy in the presence of a catalyst is 60.5 kJ "mol"^(-1) . The slop of the plot of In k (sec^(-1)) against 1/T in the absence of catalyst is :

On introfucing a catalyst at 500K , the rate of a first order reaction increases by 1.718 times. The activation energy in the presence of a catalyst is 4.15 KJ mol^(-1) . The slope of the polt of k(s^(-1)) against 1//T in the absence of catalyst is