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

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

Given:

**k** = .**1 × 10 ^{−8} s**

**E _{a}** = 261 kJ/mol =

**R** = **8.314 J/mol • K**

**T** = 325 °C + 273.15 = **598.15 K**

**A** = ?

The rate constant at 325 °C for the decomposition reaction C_{4}H_{8} ⟶ 2C_{2}H_{4} is 6.1 × 10^{−8} s ^{−1}, and the activation energy is 261 kJ per mole of C_{4}H_{8}. Determine the frequency factor for the reaction.

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