1. Chem I: 5.5.16 Due: Stoichiometry Lab
Stoichiometry Packet-still missing a few
Objectives:
Stoichiometry Exam
Energy Review and Introduction to Reaction Rates
Homework:
Energy/Reaction Rate Assignment

2. Stoichiometry: Limiting Reactants
Limiting Reactant: completely consumed during a chemical reaction.
Excess Reactant: partially consumed during a chemical reaction
en.wikipedia.org

3. Chem I: 5.9.16 Due: Stoichiometry Lab-some are missing
Stoichiometry Packet-still missing a few
Objectives:
Practice Chemistry Cumulative Exam
Energy Review and Introduction to Reaction Rates
Homework:
Reaction Rates

4. Thermochemistry
Study of how energy flows between matter during physical and chemical changes.
Energy is not classified as matter because it does not have a volume or mass.
Energy always flows from hot to cold to matter.
Energy flow can be measured using a thermometer.
Units for Energy: Joules (J) or calories (cal).

5. Heat Energy Flow Energy flows between: The System:
The matter you are studying/measuring.
The Surrounding :
The matter( the environment) around the system.
Energy Processes:
Endothermic Process:
When more heat is absorbed by the system.
Exothermic Process:
When more heat is released by the system. 5

6. Chem I: 5.11.16 Due: Thermochemistry Packet (front page) Objectives:
I can understand how energy is associated with changes that matter undergoes.
I can classify changes as endothermic and exothermic.
Homework:
Reaction Rates

9. Chemical Energy Potential Chemical Energy:
Energy absorbed by system during chemical and physical changes.
Stored in the chemical bonds.
Causes bonds to break.
Kinetic Energy:
Energy released by system during chemical and physical changes.
Produced during formation of bonds (more stable).
Influences the movement of particles in a system.
Amount can be measured using a thermometer.

10. Energy Changes: Thermometer
Energy changes between the system and its surroundings can be measured using a thermometer.
(Energy changes = Temperature changes)
Temp. change indicates a change in speed of particles of system or surroundings (kinetic energy)
Primary unit of measurement by scientists:
Celsius (oC) and Kelvin (K) scales

11. Chemical Reaction Energy Diagram
Explain using data from graph whether or not this is an endothermic or exothermic
reaction.
(Potential)

12. Chemical Reaction Energy Diagram a
Explain using data from the graph whether is an endothermic or exothermic
reaction.
Activation
Energy
(Potential)

13. Endothermic Reactions
Energy absorbed by system > Energy released
Chemical reaction gets warmer and its surroundings gets cooler.
Energy is on the reactant side.
Decomposition Reactions
Ex. Photosynthesis

14. Exothermic Reaction Energy absorbed by system < Energy released.
The chemical reaction becomes cooler and its surroundings gets warmer.
Energy is on the product side.
Synthesis and Combustion reactions
C8H O > CO2 + H2O + energy

15. Chem I: 5.12.16 Due: Thermochemistry Worksheet Objectives:
I can understand how energy is associated with changes that matter undergoes.
I can classify changes as endothermic and exothermic.
I can predict how factors influence the rate of a reaction.

16. Endo or Exo Reactions 1. H2O + energy ---> H2 + O2
2. C4H O > CO2 + H2O + energy
3. Cl KBr > KCl Br2 + energy
4. K F2 ---> KF + energy
5. Li(OH) H2(SO4) ----> Li2(SO4) + H2O

17. Chemical Reactions Rates
Reaction Rates = how fast the reactants chemically change into products.
Collision Theory: Reactant particles will form products when reactants collide:
at the right orientation(position)
and exchange the right amount of energy.

18. Chem I: 5.16.16 Due: Thermochemistry Worksheet Objectives:
I can understand how energy is associated with changes that matter undergoes.
I can classify changes as endothermic and exothermic.
I can predict how factors influence the rate of a reaction.
I can understand what chemical equilibrium is for a system.
Thermochemistry Quiz-Wednesday

19. Chemical Reactions Rates
Reaction Rates = how fast the reactants chemically change into products.
Collision Theory: Reactant particles will form products when reactants collide:
at the right orientation(position)
and exchange the right amount of energy.

20. Reaction Rates
Activation
Energy
(Potential)

21. Rates of Chemical Reactions
Identify four factors that can influence the rate of a chemical reaction.

22. Rates of Chemical Reactions
Predict how the following factors will influence the rate at which a reaction occurs based on the collision theory.
Factors
Reactants collide more or less?
Reaction Rate increase or decrease?
Increase Temperature
Increase Concentration
(amount) of Reactants
Increase Pressure
Increase Surface Area of Reactants
Add a Catalyst
Add an Inhibitor

23. Reaction Rates
Activation
Energy
(Potential)

24. Catalyst and Energy Change

25. Inhibitors Inhibitors slow down a chemical reaction.
Inhibitors bind to a catalyst and prevent it from speeding up a reaction.
Ex. Preservation of food. Antioxidants prevent foods from becoming stale or moldy.

26. Chem I: 5.18.16 Due: Thermochemistry Worksheet
Chemical Equilibrium Worksheet
Objectives:
I can understand how energy is associated with changes that matter undergoes.
I can classify changes as endothermic and exothermic.
I can predict how factors influence the rate of a reaction.
I can understand what chemical equilibrium is for a system.

27. Reaction Rates
Activation
Energy
(Potential)

28. Chemical Equilibrium

29. Reversible Reactions
What does this graph tell you about reversible reactions?

30. Reversible Reactions

31. Chem I: 5.19.16 Due: Thermochemistry Worksheet
Chemical Equilibrium Worksheet
Objectives:
I can understand how energy is associated with changes that matter undergoes.
I can classify changes as endothermic and exothermic.
I can predict how factors influence the rate of a reaction.
I can understand what chemical equilibrium is for a system.

32. Chem I: 5.20.16 Due: Chemical Equilibrium Worksheet Objectives:
Thermochemistry Quiz
I can understand how energy is associated with changes that matter undergoes.
I can classify changes as endothermic and exothermic.
I can predict how factors influence the rate of a reaction.
I can understand what chemical equilibrium is for a system.

33. Chemical Equilibrium
What factors can affect chemical equilibrium?

34. Chem I: 5.23.16 Infinite Campus: Stoichiometry Exam Due:
Thermochemistry Worksheet
Objectives:
Thermochemistry Quiz
I can understand how energy is associated with changes that matter undergoes.
I can classify changes as endothermic and exothermic.
I can predict how factors influence the rate of a reaction.
I can understand what chemical equilibrium is for a system.

35. Chemical Equilibrium What factors can affect chemical equilibrium?
-Concentration of substances in the reversible reaction.
-Temperature
-Pressure
LeChatelier’s Principle:
-If a stress is exerted on system in equilibrium, the system changes in a way to relieve that stress.
-The equilibrium position will change.

36. Changes in Chemical Equilibrium
1. Using Le Chatelier’s Principle, explain how the equilibrium position of this reaction is affected by the following changes?
N2O4(g) + 58J > 2NO2(g)
Addition of heat:
b. Decrease in pressure :
c. Addition of NO2:
d. Removal of N2O4(g):

38. Final Exam Schedule Time Thursday May 26th Friday May 27th Tuesday
Wednesday
June 1st
7:30-8:54
1st Period
1st Period Exam
9:00-10:32
2nd period
3rd Period Exam
2nd Period
2nd Period Exam
10:38-11:03
SWAMP
11:09-12:55
4th Period
4th Period Exam
1:01-2:35
5th Period
6th Period Exam
5th Period Exam