Final answer:
The activation energy for the reaction, given in the question, is 66.90 kJ/mol. It represents the energy barrier that must be overcome for the reaction to occur.
Step-by-step explanation:
The question is asking to determine the value of the activation energy (in kJ/mol) for a chemical reaction. Activation energy is defined as the minimum amount of energy required for a reaction to occur. It is often denoted by the symbol Ea.
The value provided in the question is 66.90 kJ, which is the energy barrier that the reactants must overcome for the reaction to proceed. The activation energy is a critical factor in understanding reaction rates and mechanisms, as it helps to quantify the sensitivity of a reaction to temperature changes and the presence of catalysts.
The student should note that the activation energy can also be calculated from the slope of a plot of the natural logarithm of the reaction rate constant against the inverse of the temperature, as represented by the Arrhenius equation.
However, in this question, the activation energy is directly given as 66.90 kJ/mol, and no further calculation is required.