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What is the activation energy of a reaction whose rate constant doubles when the temperature is increased from 300K to 350K (assuming that the activation energy and pre-exponential factor are both temperature independent)? Express your answer as a number with units.

Respuesta :

keziakh004

Answer:

12.1 kJ

Explanation:

For this problem, we are going to use the Arrhenius Equation.

[tex]ln(\frac{k_{2} }{k_{1}})=\frac{E_{a} }{R} (\frac{1}{T_{1}} -\frac{1}{T_{2}} )\\ln(\frac{2}{1} )=\frac{E_{a} }{8.314} (\frac{1}{300}-\frac{1}{350} )[/tex]

We are going to solve for activation energy, [tex]E_{a}[/tex].

[tex]E_{a} =12.1[/tex] kJ

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