1. Agenda
-Warm-up
-Dry-erase practice
-Chem Rxns notes
-Practice worksheet
Warm-Up
Think back to the popcorn lab…What law were you proving and how did the lab prove it?
This back to the Alka-Seltzer Lab…how did you increase the rate of the reaction (the top popping off?)

2. Dry Erase Practice

3. Counting Atoms
3NaOH
4CO2
2Fe2O3
5NaCl

4. Practice Balancing Reactions
Zn + HCl ---> ZnCl2 + H2
S8 + O2 ---> SO3
Sb O > Sb4O6

5. H3PO4 ---> H4P2O7 + H2O Zn + HCl ---> ZnCl2 + H2
Al2(SO4)3 + Ca(OH)2 ---> Al(OH)3 + CaSO4
S8 + O2 ---> SO3
FeS2 + O2 ---> Fe2O3 + SO2

6. -Potential NRG diagram wksht
WarmUp
Determine the type of chemical reaction and predict the product: H2 + O2 
H2 + Cl2  2HCl
How many grams of HCl can be produced if 7.25 g of Cl2 is reacted H2?
Agenda:
-WarmUp
-Review Hmwk
-Endo vs Exo notes
-Potential NRG diagram wksht
--Exit Slip

7. Endothermic Vs. Exothermic Reaction Graphs

8. Collision Theory
the more collisions in a system, the more likely combinations of molecules will happen.
It is the correctly aligned collisions that allow for chemical reactions to occur

10. What is activation energy?

11. Activation Energy
The lowest amount of energy particles must have in order to react
Particles must hit at precisely the right way, otherwise they will not react with one another

12. What is the activation energy for the forward reaction?

13. What is the activation energy for the reverse reaction?

14. More Questions…
What is the enthalpy change (ΔH) of reaction for the forward reaction?
What is the enthalpy change (ΔH) of reaction for the reverse reaction?

15. Endothermic Vs. Exothermic Reaction Graphs
Endothermic Reaction: a reaction in which the products have more stored energy than the reactants.
The reaction ABSORBS energy from the surrounding environment and the products use up this energy to create chemical bonds. The products are colder than the reactants.

16. Endothermic Vs. Exothermic Reaction Graphs
Exothermic Reaction: a reaction in which the products have less stored energy than the reactants.
The reaction RELEASES energy when bonds are broken. The products are hotter than the reactants.

17. Exothermic Reaction Graph
Activation Energy-the energy needed to start a reaction
Energy stored in the Reactants E N R G Y
Energy released in the reaction
Energy Stored in the Products
TIME

18. Endothermic Reaction Graph
Activation Energy-the energy needed to start a reaction
Energy Stored in the Products
Energy stored in the Reactants E N R G Y
Energy absorbed in the reaction
TIME

19. What factors affect the speed of a reaction?

20. What does rate of reaction mean?
The speed of different chemical reactions varies hugely. Some reactions are very fast and others are very slow.
The speed of a reaction is called the rate of the reaction.
What is the rate of these reactions?
rusting
explosion
baking

21. Chemical Reaction Rates
Factors that affect the rate of chemical reactions
Temperature
Concentration
Surface area
Catalyst

22. Temperature
Temperature—increase in temperature, chemical reaction rate increases.
Increase in temperature means there is an increase in collisions and a faster reaction rate.

23. Concentration
Concentration—the more concentrated a substance is, the faster a chemical reaction takes place.
More concentrated means there are more particles per unit volume.

24. Surface Area
Alka-Seltzer?
Surface Area—greater the surface area, increase in reaction rate.
Greater surface area—smaller particles

25. Catalyst
Catalyst—speeds up a reaction without permanently changing itself.
Lowers the amount of energy needed to start a reaction.

26. -Review worksheet from previous class
Agenda:
-Warm-Up
-Review worksheet from previous class
-Begin test review
Warm-Up
Explain what two things are needed for a chemical reaction to occur.
Explain what a catalyst is.
What is the activation energy of the forward reaction?