​Kinetics & Equilibrium

Kinetics and Equilibrium (Chapter 8 in text pages 136-150)

Definitions
 
Kinetics
Collision Theory
Activated complex
Activation energy
Catalyst
Potential energy diagrams
Endothermic
Exothermic
Heat of Reaction
Enthalpy
Entropy
Equilibrium
Stress
Le Chatelier’s principle
 
 
Targets:

1. I can use the Collision Theory to explain how reactions occur. 
   1. To be an effective collision particles must collide with
      1. Proper orientation
      2. Sufficient energy
2. I can identify factors that affect the rate of reaction as: nature of reactants (ionic faster), concentration (more of a substance, better chance for collisions), temperature (faster particles move the better the chance of collisions), surface area (powder always faster than block), catalyst (speeds up reaction without being used), pressure (only affects gases).
3. I can use Potential Energy diagrams to show energy and reactions (endothermic vs exothermic).
   1. I can draw and identify
      1. PE reactants
      2. PE products
      3. PE activated complex
      4. Activation Energy
      5. Heat of Reaction
      6. Catalyst path
4. I can calculate the Heat of Reaction by subtracting the PE of the Products from the PE of the Reactants.
   1. Negative value is exothermic
   2. Positive value is endothermic
5. I can predict spontaneity of reactions using enthalpy (heat of reaction) and entropy (randomness or disorder in a system) because reactions tend to go toward LESS ENERGY and MORE DISORDER.
6. I can define an equilibrium reaction as one that takes place in a CLOSED system; one in which the Forward = Reverse RATES; one that has CONSTANT CONCENTRATIONS.
7. I can identify equilibrium reactions as PHASE, SOLUTION or CHEMICAL equilibrium.
8. I can identify stress in a system and use LeChatelier’s Principle to show how the system would adjust to the stress to reestablish equilibrium.