One common method for calculating activation energy is through the use of the Arrhenius equation: \[ k = A \cdot e^{-\frac{E_a}{RT}} \] where: - \( k \) is the rate constant, - \( A \) is the pre-exponential factor, - \( E_a \) is the activation energy, - \( R \) is the universal gas constant, - \( T \) is the temperature in Kelvin.
By plotting the rate constant (\(k\)) against the inverse of temperature (\(\frac{1}{T}\)), one can determine the activation energy from the slope of the line, which is equal to \(-\frac{E_a}{R}\).
