Activation energy can be determined experimentally using the Arrhenius equation: \[ k = A e^{-Ea/RT} \] where \( k \) is the reaction rate constant, \( A \) is the pre-exponential factor, \( Ea \) is the activation energy, \( R \) is the gas constant, and \( T \) is the temperature in Kelvin. By plotting \( \ln(k) \) versus \( 1/T \), the slope of the resulting line can be used to calculate the activation energy.
