Q.Write the Arrhenius equation and explain the terms.

The Arrhenius equation quantitatively relates the rate constant of a reaction to temperature and activation energy through an exponential (Boltzmann-type) factor.

Equation:

$k = A\,e^{-E_a/RT}$

Terms explained:

• $k$: the rate constant of the reaction at temperature $T$.
• $A$: the Arrhenius factor or pre-exponential (frequency) factor — a constant for a given reaction that represents the frequency of collisions between reacting molecules and accounts for the fraction of collisions that are correctly oriented (steric factor). It has the same units as $k$.
• $E_a$: the activation energy — the minimum extra energy (over and above the average energy of reactants) that colliding molecules must possess for the collision to result in a chemical reaction (formation of the activated complex).
• $R$: the universal gas constant, $8.314\ \text{J K}^{-1}\text{mol}^{-1}$.
• $T$: the absolute temperature in Kelvin.

Logarithmic (linear) form, useful for graphical determination of $E_a$ and $A$:

$\ln k = \ln A - \dfrac{E_a}{RT}$

or, in base-10 form: $\log k = \log A - \dfrac{E_a}{2.303\,RT}$

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