Problem: The activation energy of a reaction is 56.8 kJ/mol and the frequency factor is 1.5 x1011/s. Calculate the orientation factor of the reaction at 25°C.A. 17 s-1B. 34 s-1C. 2.1 x 10-9s-1D. 6.3 x 103s-1E. none of these

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 1.5x10¹¹ s^-1

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

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

where k = is the rate; 

A = Frequency factor

Ea = Activation energy

R = Gas constant

T = Temperature