Reaction Rates

1. Reaction Rates Section 6.3

2. Activation Energy • There is a certain amount of energy needed in order for a chemical reaction to occur • The energy comes from the kinetic energy of the moving particles • If the collide with enough force to overcome the potential energy in the chemical bonds, the reaction starts • The energy needed when the particles collide is called Activation energy

3. Amount of Activation Energy • Each reaction requires a different amount of activation energy • Some reactions, like potassium and water, will occur when two substances are put in contact with one another • Other reactions, like the combustion of propane, need some energy to get started and then will continue without the added energy

4. Reaction Rates • All reactions occur at different rates • There are two different methods for measuring the rate of a reaction • Disappearance of the reactants • Appearance of the products • In each of these methods the rate is determined by how fast these things occur

5. Effecting Rates of Reaction • Increasing temperature increases the rate of reaction • Increasing concentration increases the rate of reaction • Increasing pressure (decreasing the amount of space for the reaction to occur) increases the rate of reaction • Adding a catalyst increases the rate of a reaction

6. Catalysts • Make sure to find out all you can about catalysts