The slope of a line in the graph of log k versus `1/T` for a reaction is `-5841`K. Calculate energy of activation for the reaction.

Explanation

To solve the problem, we will use the Arrhenius equation, which relates the rate constant \( k \) to the temperature \( T \) and the activation energy \( E_a \):

\[ k = A e^{-\frac{E_a}{RT}} \]

Taking the natural logarithm of both sides, we get:

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