```
k = Ae^(-Ea/RT)
```
where:
* k is the rate constant
* A is the pre-exponential factor
* Ea is the activation energy
* R is the ideal gas constant
* T is the absolute temperature
The activation energy (Ea) represents the minimum energy required for the reactants to reach the transition state and form products. As temperature increases, the average kinetic energy of the reactant molecules also increases, leading to a higher probability of collisions with enough energy to overcome the activation energy barrier. Therefore, the rate constant (k) increases exponentially with temperature.
This relationship between temperature and reaction rate is observed experimentally and has significant implications in various fields, such as chemical engineering, industrial processes, biochemistry, and environmental chemistry.
