Activation Energy: The Spark That Starts a Reaction

Activation energy is the minimum energy molecules need to collide and react.
It acts like a “start-up cost” before a chemical change can happen.
Striking a match works because friction provides the activation energy for combustion.
High activation energy means a reaction is slow unless extra heat or a catalyst is added.
Low activation energy lets reactions occur rapidly, sometimes explosively.
Catalysts lower activation energy, making reactions easier without being used up.
Enzymes in your body slash activation barriers, keeping life’s chemistry running fast.
Activation energy explains why wood doesn’t burst into flames at room temperature.
Graphs of reactions often show a hill—the peak is the activation energy barrier.
Without activation energy, the world would be full of uncontrolled, runaway reactions.