Collision Theory says that....
A chemical reaction can only happen if two particles collide with sufficient energy (called the activation energy)
What does this mean? Well it's pretty simple really!
A + B --> C
If particles A and B collide with each other, there is one of two possible outcomes!
1. They collide with an energy less than the activation energy. In this case, they just bounce off each other and nothing happens!
2. They collide with an energy equal to or greater than the activation energy. In this case, we call it a SUCCESSFUL COLLISION and a reaction takes place.
The higher the frequency of successful collisions, the faster the rate of the reaction!
Every chemical reaction has its own activation energy. They are all different.
How can I change the rate of a chemical reaction?
There are four different factors you need to know about, that can alter the rate of a chemical reaction. We will look at the explanation for each on a different page!
1. Changing the surface area of a solid
2. Changing the concentration of a solution (or pressure for a gas)
3. Changing the temperature
4. Using a catalyst
Click on each link above to see....