Chemistry
Activation Energy
Quick fact
Adding a catalyst can lower the activation energy, making reactions occur much faster without changing the overall energy change.
Why this is interesting
Have you ever wondered why some reactions happen instantly while others take years? It all starts with a hidden energy barrier called activation energy.
Read the full explanation
Understanding Activation Energy
Imagine two people trying to push a heavy box. They need enough strength (energy) to get it moving. Similarly, molecules must have enough energy to overcome an 'energy barrier' before they can react. This minimum energy is called activation energy.
A deeper explanation
Activation energy is the energy required for reactant molecules to collide with sufficient force and orientation to break existing bonds and form new ones. It acts as a threshold that determines how quickly a reaction proceeds. Even if a reaction is thermodynamically favorable, it may not occur without enough activation energy. This concept explains why temperature increases often speed up reactions—higher temperatures provide more kinetic energy to the molecules.