Given the following data for the reaction A $\to$ B,determine the activation energy,E_a,of the reaction.

Question

Quizplus · Accepted Answer

The activation energy is the difference in energy between the reactants and the transition state. The transition state is the highest energy point on the reaction pathway. The activation energy can be determined from the Arrhenius equation:k = Ae^(-Ea/RT)where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature.The data in the table can be used to plot a graph of ln(k) vs. 1/T. The slope of this graph is -Ea/R. The activation energy can then be calculated from the slope of the graph.The slope of the graph is -0.0022 J/mol/K. Therefore, the activation energy is:Ea = -slope * R = -(-0.0022 J/mol/K) * 8.314 J/mol/K = 370 J/mol

Given the Following Data for the Reaction A →\to→ B,determine the Activation Energy,Ea,of the Reaction

Given the Following Data for the Reaction A $\to$ B,determine the Activation Energy,E_a,of the Reaction