1. Unit 1: Reaction Kinetics
Lesson 2: Reaction Rates and How to Change Them

2. Where were we...?
We left off looking at how to measure reaction rates. We graphed mass vs. time and noted that you could also use properties such as temperature, gas pressure, or colour intensity to determine reaction rate.
Today we’ll look more closely at a reaction rate graph...

3. Average and Instantaneous Reaction Rates
Explain shape of graph, then show how to find each type – 5 min.

4. Your Turn!
Pg. 11 #18 and 19a,b.
5 min

5. Brain Break!

6. Collision Theory
In order to react, two molecules must collide with sufficient energy and correct geometry.
A collision that results in a reaction is referred to as an effective collision.
Collision theory can help us understand why certain factors affect reaction rates...
Use velcro balls to demonstrate! – 5 min

7. Factors Affecting Reaction Rates
1) Temperature: Temperature is a measure of the average kinetic energy of the particles in a substance. Thus, if temperature increases, the particles have more kinetic energy, so they move faster. This causes them to collide more often and with more energy, which increases the reaction rate.
Notes, then demo with velcro balls (slow then fast, timing each) – 10 min

8. Factors Affecting Reaction Rates
2) Concentration Recall that concentration (usually mol/L) is a measure of the number of particles in a given amount of space. If the concentration of a reactant increases, then there are more particles in a given amount of space. Thus the particles will collide more often, so the reaction rate increases.
Notes, then demo (fewer, then more, timing it) – 10 min

9. Factors Affecting Reaction Rates
3) Pressure Pressure is really just the concentration of a gas – the number of gas particles in a given amount of space. Thus pressure has the same effect on reaction rate as concentration does – when the pressure increases, the reaction rate increases (and vice versa).
5 min

10. Homework:
Pg. 11 #18 and 19a,b (if not already finished) and pg. 10 #17.