Question

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.

Answer 1

Answer:

12.1 kJ

Explanation:

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

$ln(\frac{k_{2} }{k_{1}})=\frac{E_{a} }{R} (\frac{1}{T_{1}} -\frac{1}{T_{2}} )\\ln(\frac{2}{1} )=\frac{E_{a} }{8.314} (\frac{1}{300}-\frac{1}{350} )$

We are going to solve for activation energy, $E_{a}$.

$E_{a} =12.1$ kJ