Rates of Reaction

1. Rates of Reaction

2. Rates of Reaction • Reactions occur because there are successful collisions between reactant particles, i.e. they collide in the correct direction and with enough energy. • If they do not have enough energy, they are dud collisions. • Anything that increases the frequency of these collisions will increase the rate.

3. Rates of Reaction • The Kinetic Molecular Theory

4. Rates of Reaction • The rate is a measure of how fast the products are made or reactants are used up

5. Rates of Reaction • There are four important factors that influence the rate of reaction that you need to know about: • Concentration • Surface area • Temperature • Catalysts

6. Rates of Reaction Concentration • Doubling the concentration will double the number of particles and hence double the chance of successful collisions, therefore the reaction should take half the time and the rate should be twice as fast

7. Rates of Reaction Surface area • The more particles that are exposed, the higher the frequency of successful collisions therefore faster the rate

8. Rates of Reaction Temperature • This gives particles more energy so they collide with more energy and more frequently. This increases rate as there are more successful collisions

9. Rates of Reaction Catalyst • This provides a surface for the reaction to take place on and hence increases the frequency of collisions.