Question

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

Answer 1

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=zpe^(-(Ea)/(RT))`

where,
`k` is the rate constant,
`z` is the collision factor,
`p` is the steric factor,
`Ea` is the activation energy,
`R=8.3245J/(mol.K)` is the ideal gas constant
and `T` is the temperature.

The Arrhenius equation could also be written as: `k=Ae^(-(Ea)/(RT))`,

where, `A=zp` is the Arrhenius factor.

Taking the natural logarithm of both parties, we get:

`lnk=-(Ea)/R(1/T)+lnA`

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.