1. Kinetics and Equilibrium

2. Kinetics
The study of the mechanisms of a reaction and the rates of reaction.
****** A reaction is at Equilibrium when:
The rate of the forward reaction is EQUAL to the rate of the reverse reaction

3. Kinetics
The study of the mechanisms of a reaction and the rates of reaction.
****** A reaction is at Equilibrium when:
Concentration of Reactants and Products are CONSTANT NOT EQUAL!!!!!!!!!!!!!!!!!!!!!!

4. Factors that effect Rate of Reaction (R of R)
Collision Theory
Anything that will increase the number of and frequency of the collisions
More effective collisions

5. Factors that Effect Rates of Reactions (T,A,P,S,C,N)
Temperature -(Average Kinetic Energy=motion)
Inc. Temperature = Increase R of R
Amount
Increase Amount (concentration) = Increase R of R
Pressure (g only) - Inc Pressure = increase R of R
Surface Area – Inc. S.A. = Inc. R of R
Nature of Reactants (Ionics > Covalents)
Due to their reactivity and the number of bonds needed to break

6. Catalyst – anything that is added that will increase
the R of R
If present will increase the R of R How?
By providing an alternative pathway for the Reaction by effecting (Lowering) 3 things
Ea of the Forward Catalyzed Reaction
Ea of the Reverse Catalyzed Reaction
PE of the Activated complex

7. Two Kinds of Reactions Endothermic Absorb Energy Heat + AB  A +B
Heat is a reactant
Break Bonds
+ H
Exothermic
Release Energy
A + B  AB + Heat
Heat is a product = Stability
Bond formation H

8. (Most Effective Collisions)

10. PE of the Activated Complex (Most Effective Collisions)
PE of the Reactants
PE of the Products
PE of the Activated Complex (Most Effective Collisions)
Ea =Activation Energy of forward Rxn
(The minimum amount of energy needed to start a reaction to completion)
Ea of the Reverse Rxn
NOTE: Endo > Exo therefore Exo is more spontaneous
H (Heat of Reaction- Enthalpy)
H = Hproducts – Hreactants H = Endothermic
H = Exothermic

16. Entropy S
Entropy is defined as the degree of
randomness, disorder, chaos
(s) – (l) – (aq) – (g)

17. Gibbs Free energy G
A reaction will always proceed spontaneously if the sign for Gibbs free energy is (-) G
The two conditions that favor a G
are : low energy H Exothermic
high entropy S

18. LeChatelier’s principle
States that when a system that is at equilibrium is placed under a stress, the systems equilibrium will shift in order to relieve the stress
Inc. (T) : will always favor endothermic reactions
Inc (P) : will always favor the side of less mole formation

19. A + B C + D
Equilibrium

21. N2
3H2
NH3
HEAT

22. CH4
3H2
CO2
H2O
HEAT