1. Reaction Rates and Equilibrium
Chapter 16

2. 16.1 Expressing Reaction Rates
rates are expressed as a change in quantity (concentration) over a change in time
the rate of a chemical reaction is defined as the change in concentration of a reactant or product per unit time, expressed as mol/(Ls)

3. Expressing Reaction Rates
Reaction rates must always be positive!
If you’re measuring the disappearance of a reactant then you use a negative sign to show that the concentration is decreasing.

4. The Collision Theory
The collision theory states that atoms, ions, and molecules must collide in order to react.
Only a small fraction of collisions produce reactions! How could this be?
Particles must have the right orientation and the right energy for a reaction to happen!

5. Collision Theory
When the orientation of two colliding molecules is correct, a reaction occurs in which an intermediate substance is formed.
activated complex or transition state
It is subsequently consumed and does not show up in the overall reaction.

6. Collision Theory
Particles must have a minimum amount of energy to form the activated complex and to lead to a reaction.
A high activation energy leads to a low reaction rate.
A low activation energy means that more particles will have enough energy to react, so reaction rate is high (fast).

7. Summary of Collision Theory
Reacting substances (atoms, ions, or molecules) must collide.
Reacting substances must collide with the correct orientation.
Reacting substances must collide with sufficient energy to form the activated complex.

10. Homework After reading 16.1, you should be able to do the following:
P. 586 (45-49)

11. 16.2 Factors affecting rates
Nature of Reactants - reactivity
Temperature-Kinetic energy is affected
Concentration-More frequent collisions
Surface Area – size of particles
Particle size- Greater surface area
Catalysts- Lower the activation energy

13. Catalysts and Inhibitors
Inhibitors slow down the reaction rate or prevent it from happening at all!
Heterogeneous catalysts are in a different physical state than the reactions they catalyze.
Homogeneous catalysts are in the same state.

14. Homework After reading 16.2, you should be able to do the following:
P. 586 (54-58)

15. 16.3 Reaction Rate Laws
The equation that expresses the relationship between the rate of a reaction and the concentration of reactants is called a rate law.
For the reaction A  B the rate law is rate = k[A]
where k is the specific rate constant

16. Rate Law Constant Units for the rate constant may be:
L/(mol s), L2/(mol2 s), or s-1
k is unique for every reaction and depends on temperature!
k does not change with concentration

17. Reaction Order
The reaction order for a reactant defines how the rate is affected by the concentration of that reactant.
First order: doubling the reactant concentration doubles the rate
Second order: doubling the reactant concentration quadruples the rate

18. Reaction Order For the reaction: aA + bB  cC The general rate law is:
rate = k[A]m[B]n
where m and n are the orders for A and B
For example: 2NO + 2H2  N2 + 2H2O has the rate law: rate = k[NO]2[H2]
Which reactant is first order? Second order?
What is the overall reaction order?

19. Determining Reaction Order
Look at Trials 1 & 2: What happens when [A] is doubled?
Look at Trials 2 & 3: What happens when [B] is doubled?
What would be the rate law for this reaction?

20. Homework
P. 587 (62,63,66-68)

21. Entropy Calculations ΔS˚ = S˚(Products)- S˚(Reactants)
S˚= standard entropy, page 558

22. Free Energy Calculations
ΔG = ΔH – TΔS
Δ G˚ = Δ G˚f (Products)- Δ G˚f (Reactants)