1. 6.3 Nature of Reactions Objectives
Demonstrate factors that influence the directions of a reaction.
Classify factors that influence the rate of a reaction.

2. Reversible Reactions Many reactions can change direction.
These reactions are called reversible reactions.
They are reversible based on energy flow.
However, not all reactions are reversible
Formation of caves, drying of paint and the burning of fuel.

3. Automobile Battery
Pb(s) + PbO2(s) + 2 H2SO4(aq) PbSO4 (s) + 2 H2O(l) + energy
When a car isn’t running the battery releases the energy as it moves to the right.
If you need to jump start the battery the reaction moves to the left while the car engine runs

4. Equilibrium
Equilibrium – term for a system where no net change occurs in the amount of reactants or products
Dynamic Equilibrium – term describing a system in which opposite reactions are taking place at the same rate.

5. Reactions at Equilibrium
Reactants are never used up, b/c they are constantly being formed by the products
Reactants and products are being formed at the same rate.
Example-Lime
CaCO3(s) CaO(s) + CO2(g)
Reactions at equilibrium do not necessarily have the same amount of reactants and products

6. Changing Direction
Le Chatelier’s principle-disturbing an equilibrium will make a system readjust to reduce the disturbance and regain equilibrium.
Chemical engineers apply this to obtain a larger product yield
They will remove some product so the reaction will produce additional product in order to reach equilibrium.

7. CaCO3(s) CaO(s) + CO2(g)
If carbon dioxide is removed as it is produced the reaction will produce more to achieve equilibrium
When one produce is a gas and the other products and reactants are not, it is easy to see how the gas can be removed
A product that does not dissolve in water can be removed if all other products and reactants dissolves in water.
Soluble-it dissolves in a liquid
Insoluble-does not dissolve in a liquid
An insoluble product will form a precipitate and sink to the bottom

8. Adding Reactants or Energy
Adding more reactants has the same effect as removing products
Adding or removing energy (usually as heat) can also influence the direction of a reaction
Because energy is part of any reaction it can thought of as either a reactant or a product

9. 3 C + 2 Al2O3(s) + energy  4 Al(l) + 3 CO2(g)
If more energy is added then the reaction goes to the right forming more aluminum and carbon dioxide

10. N2(g) + 3 H2 (g)  2 NH3(g) + energy
Adding energy to the right will cause the reaction to move to the left
This will produce more nitrogen and hydrogen

11. Reaction Rate The rate at which a reaction occurs
Activation Energy – the amount of energy the particles in a reaction must have when they collide for the reaction to occur
Reaction can be sped up or slowed down.

12. Temperature Temperature can speed up or slow down reactions
A rise in temperature caused the baking of a cake to speed up
Decreasing temperature can slow down a reaction such as keeping film cool so that film has a better self life

13. Concentration
Concentration – the amount of a substance present in a unit volume
Concentration also effects the reaction rate
A rise in concentration will increase the rate of a reaction
A decrease in concentration will slow down the reaction

14. Limiting Reactant
Limiting Reactant – the reactant of which there is not enough; when it is used up, the reaction stops and no new product is formed
Limiting reactants control the amount of product that a reaction produces, once it is used up the reaction ceases

15. Catalysts
Catalysts- a substance that speeds up the rate of a reaction without being permanently changed or used up itself
Catalysts do not change the position of equilibrium and therefore does not affect how much product is formed
Enzymes – biological catalysts
Enzymes are involved in almost every process in a cell
Figure 6.22 page 222 Jello and Pineapple

16. Slowing Down Reactions
Inhibitor – a substance that slows down a reaction
Inhibitors do not completely stop a reaction
An inhibitor is placed in bottles of hydrogen peroxide to prevent the decomposition

17. Review Define: What does a catalyst do to a reaction?
Equilibrium
Dynamic Equilibrium
Activation Energy
What does a catalyst do to a reaction?
What does a inhibitor do to a reaction?

18. Homework Page 223 #1-3 Page 225 # 7 Extra Credit:
Read page and answer #1-2
Read page 221 and answer #1-2