Rate of Reaction Basics
Ever wondered why some reactions happen instantly whilst others take ages? The rate of reaction tells you exactly how fast a chemical change occurs. You can measure it by tracking either how quickly products form or how fast reactants disappear over time.
Collision theory explains why reactions happen at all. Particles must crash into each other with enough energy to actually react - this minimum energy needed is called the activation energy. Think of it like trying to break through a brick wall - you need enough force to make it happen.
Most reactions start fast because there are loads of particles bumping into each other. As the reaction continues, fewer reactant particles remain, so collisions become less frequent and the reaction slows down. Eventually, one reactant runs out completely and the reaction stops.
Quick Tip: Remember that particles need both collision AND sufficient energy to react successfully.
