The rate constant of a chemical reaction increased from 0.100s1 to 3.00s1 upon raising the Learning Goal: temperature from 25.0C to 49.0C. To use the Arrhenius equation to calculate the activation energy. As temperature rises, the average kinetic energy of molecules increases. In a chemical reaction, this means that a higher percentage of the molecules possess the required activation energy, and the reaction goes faster. This relationship is shown by the Arrhenius equation k=AeEa/RT where k is the rate constant, A is the frequency temperature. factor, Ea is the activation energy, R=8.3145 J/(Kmol) is the gas constant, and T is the Kelvin temperature. The following rearranged version of the equation is also useful: ln(k2k1)=(REa)(T21T11) where k1 is the rate constant at temperature T1, and k2 is the rate constant at temperature T2. * Incorrect; Try Again; One attempt remaining Calculate the value of ln(k2k1) where k1 and k2 correspond to the rate constants at the initial and the final temperatures as defined in part A. Express your answer numerically. What is the activation energy of the reaction? Express your answer numerically in kilojoules per mole