The Arrhenius equation is a way to explain how the speed of a chemical reaction depends on temperature and the energy needed to start the reaction (activation energy).
Key points:
- Higher temperature → particles move faster → more collisions have enough energy → reaction goes faster.
- Lower activation energy → easier for particles to react → faster reaction.
- Frequency of collisions also affects the rate; more frequent collisions make reactions faster.
- It shows that even small changes in temperature or activation energy can have a big effect on how fast a reaction occurs.
In short: The Arrhenius concept tells us that reactions happen faster when particles collide more often and have enough energy to overcome the energy barrier.