To understand what adding a catalyst to a reaction does, let's go over each option:
1. Increase the amount of each product formed by the reaction: This statement is incorrect. A catalyst does not affect the overall amount of product formed in a reaction.
2. Lower the activation energy of the reaction: This statement is correct. A catalyst lowers the activation energy required for a chemical reaction to proceed, making it easier for the reactant molecules to overcome the energy barrier and form products.
3. Alter the orientation of reactants in the reaction: This statement is incorrect. A catalyst does not alter the orientation of reactants in a reaction. It only provides an alternative reaction pathway with a lower activation energy.
4. Increase the rate of the reaction: This statement is correct. A catalyst speeds up the rate of a chemical reaction by reducing the energy required for reactant molecules to collide effectively and form products.
So, the correct answers are:
- Lower the activation energy of the reaction
- Increase the rate of the reaction