The rate of reaction `((dx)/(dt))` varies with nature, physical state and concentration of reactants, temperature, exposure to light and catalyst, whereas rate constant `(K)` varies with temperature and catalyst only. The rate constant `K` is given as `K=Ae^(-E_(a)//RT)` where `A` is Arrhenius parameter or pre-exponential factor and `E_(a)` is energy of activation. The minimum energy required for a reaction is called threshold energy and the additional energy required by reactant molecules to attain threshold energy level is called energy of activation.
For a reaction, `Ararr B`, if
`log_(10) K (sec^(-1)) =14-(1.25xx10^(4))/(T)K`, the Arrhenius parameter and energy of activation for the reaction are:

Options

A. `10^(14)" sec"^(-1), 239.34 kJ`
B. 14,57.6 kcal
C. `10^(14)" sec"^(-1), 23.93 kJ`
D. `10^(14)" sec, "5.76` kcal

Answer

A