🤓 Based on our data, we think this question is relevant for Professor Dixon's class at UCF.

Two reactions have identical values for E_{a}. Does this ensure that they will have the same rate constant if run at the same temperature?

We have to determine if two reactions with the same activation energy would have the same rate constants if they are run at the same temperature.

We will use the **two-point form of the Arrhenius equation** to solve this problem.

$\overline{){\mathbf{ln}}\frac{{\mathbf{k}}_{\mathbf{2}}}{{\mathbf{k}}_{\mathbf{1}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{\mathbf{-}{\mathbf{E}}_{\mathbf{a}}}{\mathbf{R}}\mathbf{(}\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{2}}}\mathbf{}\mathbf{-}\mathbf{}\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{1}}}\mathbf{)}}$

**Where,**

k_{1} = rate constant at T_{1}

k_{2} = rate constant at T_{2}

E_{a} = activation energy

R = universal gas constant

T_{2} = higher temperature

T_{1} = lower temperature

Arrhenius Equation

Arrhenius Equation

Arrhenius Equation

Arrhenius Equation