The rate constant for a first order reaction is 0.060s-1. when the temperature is increased from 298K to 331 K , the rate constant increases to 0.18s-1. Calculate the activation energy for this reaction. Use kJ/mol for the units. The activation energy in kJ/mol equals (include the units in your answer):

27.3 kJ/mol

Explanation:

You would use the Arrhenius Equation to solve this problem.

Plug the rate constants into k1 and k2.  Plug the temperatures into T1 and T2. R is a constant and is equal to 8.314.  Solve for Ea.

Your answer should be 27,303.03 J/mol or 27.3 kJ/mol.

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