We could find out more information about ths reaction by studying the temperature dependence of the rate constant, k. These same experiments could be carried out at a lower temperature (ice bath) and a second rate constant, k2 could be determined for this temperature. Using the Arrhenius equation, these data could then be used to determine the activation energy, Ea, and the pre-exponential factor, A, for the reaction. The general form of the Arrhenius equation is shown below: For measurements at two different temperatures, this reduces to: ln(k2/k1) = (Ea/R)(1/T1 - 1/T2) A plot of ln k v.s. (1/T) for rate constants (k) measured at different temperatures (T) will have a slope equal to Ea/R. Substituting a value of k and the Ea into the first equation would allow you to solve for ln A. At room temperature (298 K) the rate constant for this reaction is 2.5 M-1s-1. When the experiment was repeated at 0.0oC, the rate constant was determined to be 1.0 M-1s-1. What is the activation energy, Ea for this reaction, in kJ/mol?