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**:

$\overline{){\mathbf{ln}}{\mathbf{}}{\mathbf{k}}{\mathbf{=}}{\mathbf{-}}\frac{{\mathbf{E}}_{\mathbf{a}}}{\mathbf{R}}{\mathbf{}}\left(\frac{\mathbf{1}}{\mathbf{T}}\right){\mathbf{}}{\mathbf{+}}{\mathbf{}}{\mathbf{ln}}{\mathbf{}}{\mathbf{A}}}\phantom{\rule{0ex}{0ex}}{\mathbf{y}}{\mathbf{}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{}}{\mathbf{}}{\mathbf{}}{\mathbf{}}{\mathbf{m}}{\mathbf{}}{\mathbf{}}{\mathbf{}}{\mathbf{}}\left(\mathbf{x}\right){\mathbf{}}{\mathbf{}}{\mathbf{+}}{\mathbf{}}{\mathbf{}}{\mathbf{}}{\mathbf{b}}$

where:

**m** = slope

**b** = y-intercept

The reaction

(CH_{3})_{3}CBr + OH^{- }→ (CH_{3})_{3}COH + Br^{-}

in a certain solvent is first order with respect to (CH _{3})_{3}CBr and zero order with respect to OH _{2}. In several experiments, the rate constant k was determined at different temperatures. A plot of ln(k) versus 1/T was constructed resulting in a straight line with a slope value of -1.10 x 10^{4} K and y-intercept of 33.5. Assume k has units of s^{-1}.

a. Determine the activation energy for this reaction.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.