2. Kinetics The study of the mechanisms of a reaction and the rates of reaction.

3. 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

4. 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

5. 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 3 things 1. E a of the Forward catalyzed Reaction 2. E a of the Reverse Catlayzed Reaction 3. PE of the Activated complex

6. 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

7. (Most Effective Collisions)

8. 1. PE of the Reactants 2. PE of the Products 3. PE of the Activated Complex (Most Effective Collisions) 4. E a =Activation Energy of forward Rxn 1. (The minimum amount of energy needed to start a reaction to completion) 5. E a of the Reverse Rxn 1. NOTE: Endo > Exo therefore Exo is more spontaneous 6. H (Heat of Reaction- Enthalpy) 1. H = H products – H reactants + H = Endothermic 1. - H = Exothermic

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