Arrhenius plot

Considering as example the decomposition of nitrogen dioxide into nitrogen monoxide and molecular oxygen: : Based on the red "line of best fit" plotted in the graph given above: Points read from graph: Slope of red line = (4.1 − 2.2) / (0.0015 − 0.00165) = −12,667 Intercept [y-value at x = 0] of red line = 4.1 + (0.0015 × 12667) = 23.1 Inserting these values into the form above: \ln(k) = \ln(A) - \frac{E_a}{R}\left(\frac{1}{T}\right) yields: \ln(k) = 23.1 - 12,667 (1/T) k = e^{23.1} \cdot e^{-12,667/T} as shown in the plot at the right. k = 1.08 \times 10^{10} \cdot e^{-12,667/T} for: • k in 10−4 cm3 mol−1 s−1 • T in K Substituting for the quotient in the exponent of e: E_a / R = -12\,667\,\mathrm{K} where the approximate value for R is 8.31446 J K−1 mol−1 The activation energy of this reaction from these data is then: == See also ==