We’re being asked to **determine the activation energy (E _{a})** of a reaction given that the plot of k vs. 1/T has a

We’re given the plot of k (y) vs. 1/T (x).

This means we need to use the ** two-point form of the Arrhenius Equation**:

$\overline{){\mathbf{ln}}{\mathbf{}}{\mathbf{k}}{\mathbf{=}}{\mathbf{-}}\frac{{\mathbf{E}}_{\mathbf{a}}}{\mathbf{R}}{\mathbf{}}\left(\frac{\mathbf{1}}{\mathbf{T}}\right){\mathbf{}}{\mathbf{+}}{\mathbf{}}{\mathbf{ln}}{\mathbf{}}{\mathbf{A}}}$

where:

**k** = rate constant

**E _{a}** = activation energy (in J/mol)

**R** = gas constant (8.314 J/mol • K)

**T** = temperature (in K)

**A** = Arrhenius constant or frequency factor

A plot of k versus 1/T has a slope of -7,445. What is E _{a}, for this reaction?

A, 90.79 kJ/mol

B. 895.5 J/mol

C. 304.7 kJ/mol

D. 61.90 kJ/mol

E. 610.5 J/mol

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Based on our data, we think this problem is relevant for Professor Miller's class at Utah State University.