We’re being asked to **determine the orientation factor **of a reaction given that the activation energy is 56.8 kJ/mol and the frequency factor is 1.5x10^{11} s^{-1}

Acc. to the* Arrhenius equation*, frequency factor A represents the number of approaches to the activation barrier per unit of time

$\overline{){\mathbf{k}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{{\mathbf{Ae}}}^{\mathbf{-}\mathbf{Ea}\mathbf{/}\mathbf{RT}}}$

where k = is the rate;

A = Frequency factor

Ea = Activation energy

R = Gas constant

T = Temperature

The activation energy of a reaction is 56.8 kJ/mol and the frequency factor is 1.5 x10^{11}/s. Calculate the orientation factor of the reaction at 25°C.

A. 17 s^{-1}

B. 34 s^{-1}

C. 2.1 x 10^{-9}s^{-1}

D. 6.3 x 10^{3}s^{-1}

E. none of these