Learning Goal: To use the Arrhenius equation to calculate the activation energy. As temperature rises, the...

 

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Learning Goal: 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 = Ae Ea/RT where k is the rate constant, A is the frequency factor, Ea is the activation energy, R = 8.3145 J/(K mol) is the gas constant, and T is the Kelvin temperature. The following rearranged version of the equation is also useful: In = 1 1 (*)(*)(*-*) R where k is the rate constant at temperature T1, and k2 is the rate constant at temperature T. the initial and the final temperatures as defined in part A. Express your answer numerically. View Available Hint(s) In() = 3.50 Submit Previous Answers Correct Part C What is the activation energy of the reaction? Express your answer numerically in kilojoules per mole. View Available Hint(s) Ea 183.99 = ? kJ/mol Learning Goal: 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 = Ae Ea/RT where k is the rate constant, A is the frequency factor, Ea is the activation energy, R = 8.3145 J/(K mol) is the gas constant, and T is the Kelvin temperature. The following rearranged version of the equation is also useful: In = 1 1 (*)(*)(*-*) R where k is the rate constant at temperature T1, and k2 is the rate constant at temperature T. the initial and the final temperatures as defined in part A. Express your answer numerically. View Available Hint(s) In() = 3.50 Submit Previous Answers Correct Part C What is the activation energy of the reaction? Express your answer numerically in kilojoules per mole. View Available Hint(s) Ea 183.99 = ? kJ/mol