1. Chapter 19 – Reaction Rates and Equilibrium
Rates of Reaction
Reversible Reactions and Equilibrium
Determining Whether a Reaction Will Occur
Calculating Entropy and Free Energy
The Progress of Chemical Reactions

2. 19.1 Rates of Reaction How long does a chemical reaction take?
Collision Theory
IF colliding particles have enough energy (KE) and collide at the right orientation, they react to form a new product:

3. 19.1 Rates of Reaction (cont.)
The minimum amount of energy that particles must have in order to react is called the activation energy.
Activation energy acts like a barrier that the reactants must cross to be converted into products.
Activated complex, transition state…

4. 19.1 Rates of Reaction (cont.)
Factors Affecting Reaction Rates
Here they are again…
Temperature
Concentration
Particle size
Catalysts

5. 19.2 Reversible Reactions and Equilibrium
Reactions that can occur in the other direction..
2SO2 + O SO3

6. 19.2 Reversible Reactions and Equilibrium (cont.)
Chemical Equilibrium
A state in which the forward and reversible reactions take place at the same rate.
Factors Affecting Equilibrium: Le Chatelier’s Principle
Obviously, when discussing equilibrium there is “a fine line” of balance in the reaction – changes of almost any kind can disrupt this balance.
Le Chatelier’s Principle: If a stress (temp, conc., pressure) is applied to a system in dynamic equilibrium, the system changes to relieve the stress.

7. 19.2 Reversible Reactions and Equilibrium (cont.)
Equilibrium Constants
A ratio of product concentrations…
aA + bB cC + dD
Keq = [C]c x [D]d / [A]a x [B]b
where [X] is expressed in mol/L and x is the number of moles from the balanced chemical equation.
A Keq value > 1 favors products at eq.
Keq value < 1 favors reactants at eq.
Examples…

8. Ch 19 Assignments Ch 19 CPQs #1 pg. 572
#38,39,40,41,43,44,46,47,48,49,50

9. 19.3 Determining Whether a Reaction Will Occur
Free Energy and Spontaneous Reaction
To do work, you need available energy.
Free energy: energy that is available to do work. (Not always efficient.
Reactions may OR may not occur spontaneously…
Entropy
Reactions tend to occur to attain the lowest possible energy for a system: the law of disorder.
The disorder in a system is measured as entropy, (S).

10. 19.3 Determining Whether a Reaction Will Occur (cont.)
Entropy explained and visualized…

11. 19.3 Determining Whether a Reaction Will Occur (cont.)
Entropy explained and visualized…

12. 19.3 Determining Whether a Reaction Will Occur (cont.)
Entropy explained and visualized…

13. 19.3 Determining Whether a Reaction Will Occur (cont.)
Entropy explained and visualized…

14. 19.3 Determining Whether a Reaction Will Occur (cont.)
Heat, Entropy, and Free Energy
The size and direction of heat (enthalpy) changes combined with entropy determine whether or not a reaction is spontaneous, i.e., whether it favors products and releases free energy.
Table 19.1, pg. 554

15. 19.3 Determining Whether a Reaction Will Occur (cont.)

16. 19.4 Calculating Entropy and Free Energy
Entropy Calculations
Standard entropy change (entropy change at standard conditions:
DSo = So (products) – So (reactants)
Use Table 19.2
Examples…
Free Energy Calculations
The maximum amount of energy that can be combined with another process to do work: Gibbs Free-Energy (G).
DG = DH – TDS where H = enthalpy, T = Temperature
DGo = DGof (products) – DGof (reactants)
Tables 19.3 and 19.4

17. 19.5 The Progress of Chemical Reactions
Rate Laws
Fortunately, we don’t have to settle for explanations that are qualitative in nature- in other words, “the reaction will likely favor the products…”
Mathematically calculating rates of reaction…
Rate Law: an expression relating the rate of a reaction to the concentration of reactants:
Rate = DA / Dt = k x [A]
For the reaction aA + bB cC + dD, the rate equation takes the form:
Rate = k[A]a[B]b

18. 19.5 The Progress of Chemical Reactions (cont.)
Rate Laws (cont.)
The specific rate constant,k, determines the relationship between the concentrations and the rate of reaction.
If k is large, the reaction will form products quickly.
If k is small, the reaction will form products slowly.
The order of a reaction is the power to which the concentration must be raised to give the experimentally observed relationship between concentration and rate: 1st order reaction – proportional to one reactant.
Reaction mechanisms…
Showing the reactions involved in a complex reaction
Figure 19.3, decomposition of N2O…

19. Ch 19 Assignments Ch 19 CPQs #1 pg. 572 Ch 19 CPQs #2 pg. 572
#38,39,40,41,43,44,46,47,48,49,50
Ch 19 CPQs #2 pg. 572
#51,53,54,55,56,59,61,62