Arrhenius Plots The slope and intercept of the Arrhenius...

Arrhenius Plots The slope and intercept of the Arrhenius plot for the 2$^{nd}$ order reaction of HI with CH$_3$I forming methane and iodine are -1.67 \times 10$^4$ K and 30.88, respectively. Determine the activation energy in kJ mol$^{-1}$. b = 30.88 m = -1.67x10$^4$ K

Rate constants were measured at various temperatures for the reaction, $\mathrm{HI}(g)+\mathrm{CH}_{3} \mathrm{I}(g) \longrightarrow \mathrm{CH}_{4}(g)+\mathrm{I}_{2}(g)$. The following data were obtained: $$ \begin{array}{cc}\text { Rate Constant }\left(\mathrm{L} \mathrm{mol}^{-1} \mathrm{~s}^{-1}\right) & \text {Temperature }\left({ }^{\circ} \mathrm{C}\right) \\1.91 \times 10^{-2} & 2.05 \times 10^{2} \\2.74 \times 10^{-2} & 2.10 \times 10^{2} \\3.90 \times 10^{-2} & 2.15 \times 10^{2} \\5.51 \times 10^{-2} & 2.20 \times 10^{2} \\7.73 \times 10^{-2} & 2.25 \times 10^{2} \\1.08 \times 10^{-1} & 2.30 \times 10^{2} \\\end{array}$$ Determine the activation energy in $\mathrm{kJ} / \mathrm{mol}$ both graphically and by calculation using Equation 13.16. For the calculation of $E_{\mathrm{n}}$, use the first and last sets of data in the table.

Question

Arrhenius Plots The slope and intercept of the Arrhenius plot for the 2$^{nd}$ order reaction of HI with CH$_3$I forming methane and iodine are -1.67 \times 10$^4$ K and 30.88, respectively. Determine the activation energy in kJ mol$^{-1}$. b = 30.88 m = -1.67x10$^4$ K

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