For the first order reaction `A rarr B +C` , carried out at `27^(@)` C . If `3.8 xx 10^(-16)%` of the reactant molecules exists in the activated state , the `E_(a)` (activation energy) of the reaction is:

For the first order reaction ArarrB+C , carried out at 27^(@)C if 3.8xx10^(-16)% of the reactant molecules exists in the activated state, the E_(a) (activation energy) of the reaction is :

For the first order reaction A rarr B+C carried out at 27^@C if 3.8xx10^-16 % of the reactant molecules exists in the activated state. Calculate the Ea (activation energy) of the reaction.

For the first order reaction A to B + C , carried out at 27°C, 3.8 xx 10^(-16) % of the reactant molecules exists in the activated state. The E_a (activation energy) of the reaction is:

A first order reaction is 50% completed in 20 minutes at 27^(@) C. The energy of activation of the reaction is-

The reaction A+B rarr C+D+40KJ has activation energy of "18KJ" .Then the activation energy for the reaction C+D rarr A+B is

A first order reaction is 50% complete in 30 minutes at 27^(@) C and in 10 minutes at 47^(@) C. Calculate the reaction rate constants at these temperatures and the energy of activation of the reaction in kJ//mol (R=8.314 J mol^(-1)K^(-1))

The half time of a first order reaction is 6.93 xx 10^(-3) min at 27^(@)C . At this temeprature, 10^(-8)% of the reactant molecules are able to cross-over the energy barrier. The pre-exponential factor A in the Arrhenius equation is equal to