What is the Arrhenius equation and what is meant by activation energy?

May 7, 2016

The Arrhenius equation provides a relationship between the rate constant $k$ and temperature $T$.

Explanation:

The Arrhenius equation provides a relationship between the rate constant $k$ and temperature $T$.

The Arrhenius equation is: $k = z p {e}^{- \frac{E a}{R T}}$

where,
$k$ is the rate constant,
$z$ is the collision factor,
$p$ is the steric factor,
$E a$ is the activation energy,
$R = 8.3245 \frac{J}{m o l . K}$ is the ideal gas constant
and $T$ is the temperature.

The Arrhenius equation could also be written as: $k = A {e}^{- \frac{E a}{R T}}$,

where, $A = z p$ is the Arrhenius factor.

Taking the natural logarithm of both parties, we get:

$\ln k = - \frac{E a}{R} \left(\frac{1}{T}\right) + \ln A$

The activation energy by definition, is the minimum energy (or threshold energy) required for two particles of reactants upon collision to form products.

Here is a video that fully explain this topic:
Chemical Kinetics | A Model for Chemical Kinetics & Catalysis.