Question

1. A researcher raises the temperature from 32.0 to 45.9 ⁰ C and finds that the rate of the reaction doubles. What was the activation energy (in kJ/mol) for this reaction? (R = 8.3145 J/mol K) 2. A researcher raises the temperature from 55.2 to 73 ⁰ C and finds that the rate of the reaction doubles. What was the activation energy (in J/mol) for this reaction? (R = 8.3145 J/mol K)

Answer 1

The activation energy of a reaction, which can be found using the Arrhenius equation, can be calculated using the rate constants at two different temperatures. The equation is rearranged to find the activation energy, using the data provided in the questions.

Step-by-step explanation:

In order to find the activation energy for the reactions, we can use the Arrhenius equation which states the relationship between the rate of a reaction and the temperature at which it is carried out.

It's given by the equation k = Ae-Ea/RT, where k is the reaction rate constant, A is the frequency factor, Ea is the activation energy, R is the universal ideal gas constant, and T is the temperature in Kelvin.

For the first question, converting the temperature from Celsius to Kelvin gives T1 = 305.15 K and T2 = 319.05 K. Substituting these values into the rearranged Arrhenius equation, and then solving for Ea, gives the activation energy in joules, which can be further converted to kJ to answer the first question. For the second question, using the given temperatures B1 = 328.35 K and B2 = 346.15 K in the same manner, gives the activation energy in joules.

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