Recall 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

For reactions with the following activation energies, which will have the greatest rate at 298 K? Hint: Assume that the frequency factor, A, in the Arrhenius equation is the same for each of the reactions.

A. E_{a} = 10 kJ/mol

B. E_{a} = 15 kJ/mol

C. E_{a} = 20 kJ/mol

D. E_{a} = 25 kJ/mol

E. E_{a} = 30 kJ/mol

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