1. Graphing Rates & Activation Energy
Unit 3: Reaction Rates and Equilibrium

2. Review Last Day What was collision theory?
What were the 3 factors that affect the rate of a reaction?
The rate of reaction is determined by which of these factors?

3. How do reactions take place?
If we consider the following equation,
2 C2H2 + 5 O2 → 4 CO2 + 2 H2O
This reaction says that 7 molecules (2 C2H2 and 5 O2) need to collide at once for the reaction to occur....pretty unlikely
So instead, the reaction probably occurs in two or three steps....much more likely as less molecules need to colliside properly

4. How do reactions take place?
Now take a look at this:
2 NO + O2 → 2 NO2
As we saw with Hess’s law, this may not occur all at once, but may have happened in the following steps:
1. 2 NO → N2O2
2. N2O2 + O2 → 2 NO2
The series of steps a reaction undergoes is called the reaction mechanism.
Substances that get cancelled out, like N2O2, are called reaction intermediates. These are typically short lived.

5. Activation Energy
One thing we said about collisions between molecules is that there must be enough energy between them to make a reaction.
Activation energy (Ea) is the minimum amount of energy for a successful collision. This is often called the threshold energy.

6. Activation Energy

7. Rate Determining Step
Rate Determining Step – the step that determines the overall rate of a reaction.
Just like a chain is only as strong as its weakest link, the rate of reaction depends on the slowest step.
We call the slowest step in a reaction the rate determining step. If your goal is to speed up a reaction, you want to focus on this step.

8. What is potential energy?
As particles approach each other potential energy increases.
That is, if the particles are closer together they have a greater potential to react (or do work) than if they were farther apart.
Once they hit, the potential energy is at a high

9. Transition State
If the particles hit correctly (with sufficient speed and orientation) a new ‘molecule’ will form for a very short period.
During this time, the ‘molecule’ has bonds that are both breaking and forming. Therefore, it is extremely unstable (which accounts for its short existence).
This unstable ‘molecule’ is called the activated complex, or transition state.

10. Transition State
This transition state is a combination of the two molecules coming together.
It is important to note that the molecule is not happy in this shape and wants to change quickly, hence why transition states are so short lived and why the molecule is called “unstable”.
The activation energy (Ea) is the amount of energy required to reach the activated complex.

11. Energy to Activated Complex
First let’s look at potential energy diagrams for exothermic and endothermic reactions
But there is more going on…
Recall:
∆ H is found between the energy levels of reactants and produced products

12. Energy to Activated Complex
This is what they really look like…
Note…Ea is found between the reactants and the activated complex (or transition state)

13. Energy to Activation Complex
Notes about these new potential energy diagrams:
Every reaction, even exothermic reactions, require an input of energy to reach the activation complex.
This input of energy is the activation energy.
Note the difference in the activation energy between exothermic and endothermic reactions.

14. Reaction Mechanism
Elementary reaction- a reaction that happens in a single step.
Reaction mechanism is a description of how the reaction really happens.
It is a series of elementary reactions.
The product of an elementary reaction is an intermediate.
An intermediate is a product that immediately gets used in the next reaction.

15. This reaction takes place in three steps

16. Ea
First step is fast
Low activation energy

17. High activation energyEa
Second step is slow
High activation energy

18. Ea
Third step is fast
Low activation energy

19. Second step is rate determining

20. Intermediates are present

21. Activated Complexes or Transition States

22. Example of Multi-Step Reactions
There is an activation energy for each elementary step.
Slowest step (rate determining) must have the highest activation energy.

23. Example 1
Answer the following questions about the potential energy graph below:
a. Determine the heat of reaction, ΔH, (enthalpy change) for this reaction.
Answer: 150 kJ/mol ∆H

24. Example 1
b. Determine the activation energy, Ea for this reaction.
Answer: 250 kJ/mol
∆Ea

25. Example 1
c. How much energy is released or absorbed during the reaction?
Answer: 150 kJ/mol
is absorbed
∆H released

26. Example 1
d. How much energy is required for this reaction to occur?
Answer: 250 kJ/mol Ea

27. Example 2 A - - - B - - - C A - - - B - - - C - - - D A. AB + C → BC
What do you think the following transition states would look like?
A AB + C → BC
B ABC + D → AB + CD
ANSWERS: (green is breaking; orange is forming)
A B C
A B C D