Catalysts can increase reaction rates by the activation energy, which increases the likelihood of successful collisions.

Catalysts can increase reaction rates by lowering the activation energy, which increases the likelihood of successful collisions. Here's a step-by-step explanation:

1. A catalyst is a substance that can increase the rate of a chemical reaction. It does this by providing an alternative reaction pathway with a lower activation energy.

2. The activation energy is the minimum amount of energy required for a chemical reaction to occur. It's like the energy needed to push a boulder over a hill; once it's over the hill, it can roll down the other side.

3. By lowering the activation energy, a catalyst makes it easier for the reactants to reach the energy level needed to start the reaction. This means that more of the reactant particles will have enough energy to react when they collide.

4. This increases the likelihood of successful collisions, where reactant particles collide with enough energy and in the correct orientation to react and form products. As a result, the reaction rate increases.

5. It's important to note that while catalysts increase the rate of reaction, they are not consumed in the reaction. They can be used over and over again.