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:

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

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))

A first order reaction has very high value of activation energy.

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

A first order reaction is 50% completed in 30 min at 27^(@)C and in 10 min at 47^(@)C . Calculate the reaction rate constants at 27^(@)C and the energy of activation of the reaction in kJ mol^(-1) .

A first order reaction is 50% completed in 20 minutes at 27^(@)C and in 5 min at 47^(@)C . The energy of activation of the reaction is