1. Chemistry (4/25) Objectives: Complete Chemical Quantities Exam
Perform Hydrate Lab
Homework:
Answer post lab questions.

2. Chemistry (4/26) Objectives:
Complete Hydrate Lab and post-lab questions.
Homework:
Complete post lab questions. Due Monday

3. Chemistry (4/29) Objectives:
Complete post-lab questions for Hydrate Lab.
Identify and apply stoichiometry with substances in a chemical equation.
Homework:
Stoichiometry Problems

4. Hydrate Lab Cu(SO4) . H2O ----> Cu(SO4) + H2O Post-Lab questions:
Use the equation above to help answer the following questions:
What was the hydrate salt in this experiment?
What was the anhydrous salt in this experiment?
What was the difference between the hydrated salt and the anhydrous salt in this experiment?
Was this a physical or chemical reaction? Validate your answer with data from your lab.

5. Hydrate Lab
Cu(SO4) . H2O ----> Cu(SO4) + H2O

6. Copper Sulfate Hydrate

7. What is Stoichiometry?
access.aasd.k12.wi.us

8. Stoichiometry N2 + 3H2 ----------> 2NH3 (NH3 ) (N2)

9. Chemistry (5/1) Infinite Campus Update:
Chemical Quantities Exam (37pts)
Hydrate Lab (10pts.)
Objectives:
Identify and apply stoichiometry with substances in a balanced chemical equation.
Homework:
Stoichiometry Problems

10. Bell Ringer
Calculate the percent composition of water in this hydrate: Mg(SO4) . 7H2O (Epsom Salt)
What is stoichiometry?
N2H O > N H2O
a. Balance the chemical equation.
b. How many moles of rocket fuel (N2H4) are needed to produce 8 moles of N2?

11. Bell Ringer
Calculate the percent composition of water in this hydrate: Mg(SO4) . 7H2O (Epsom Salt)
2.What is stoichiometry?
N2H O > N H2O
a. Balance the chemical equation.
b. How many moles of rocket fuel (N2H4) are needed to produce 8 moles of N2?

12. Bell Ringer
Calculate the percent composition of water in this hydrate: Mg(SO4) . 7H2O (Epsom Salt)
What is stoichiometry?
N2H O > N H2O
a. Balance the chemical equation.
b. How many moles of rocket fuel (N2H4) are needed to produce 8 moles of N2?

13. Stoichiometry N2 + 3H2 ----------> 2NH3 Stoichiometry:
Converting between substances in a balanced chemical equation using mole conversions.
(NH3)
(N2)

14. Stoichiometry H2O ----------> H2 + O2
What type of reaction is this?
Balance the chemical equation if needed.
If you start with 100 moles of H2O how many moles of H2 would be produced?
If you want to produce 3.8moles of O2, how much H2O will you need to start with?

15. Chemistry (5/2) Objectives:
Identify and apply stoichiometry with substances in a balanced chemical equation.
Homework:
Stoichiometry Problems

16. Stoichiometry: Mole to Mole

17. Stoichiometry N2 + 3H2 ----------> 2NH3 Stoichiometry:
Converting between substances in a balanced chemical equation using mole conversions.

18. Stoichiometry Problems
N2H O > N H2O
If 13.8 grams of water were produced how much rocket fuel (N2H4) in grams would have been used up?

19. Chemistry (5/6) Objectives:
Identify and apply stoichiometry with substances in a balanced chemical equation.
Homework:
Stoichiometry Problems (due Wed.)
Gas Laws Graphing Assignment (due Wed.)
Quiz: Wednesday (Stoichiometry conversions: mole to mole or grams to grams.)

20. Stoichiometry N2 + 3H2 ----------> 2NH3 Stoichiometry:
Converting between substances in a balanced chemical equation using mole conversions.

21. Stoichiometery Problems

22. Pre-AP Chemistry (4/25) Objectives:
Apply stoichiometry conversions with substances in chemical equations.
Identify and apply limiting reactants in chemical reactions.
Calculate Stoichiometry
Homework:
Stoichiometry and Limiting Reactants

23. Stoichiometry N2 + 3H2 ----------> 2NH3 Stoichiometry:
Converting between substances in a balanced chemical equation using mole conversions.

24. Stoichiometry: Limiting Reactants
Excess Reactant:
en.wikipedia.org

25. Stoichiometry: Limiting Reactants
Limiting Reactant: completely consumed
Excess Reactant: partially consumed
en.wikipedia.org

26. Stoichiometry: Limiting Reactant
HCl + Mg > MgCl H2
What type of reactions is this?
Balance equation if needed.
If 6.8 moles of Mg react with 7.5 moles of HCl which is considered the limiting reactant? excess reactant?
Reactants
Have (moles)
Need (moles)

27. Stoichiometry: Limiting Reactant
2HCl + Mg > MgCl H2
If 6.8 moles of Mg react with 7.5 moles of HCl how many moles of MgCl2 can be produced?
Reactants
Have (moles)
Need (moles)
HCl (limited)
7.5 mol
13.6
Mg (excess)
6.8 mol
3.75

28. Pre-AP Chemistry 4/26 Objectives:
Identify and apply limiting reactants in stoichiometric calculations.
Distinguish between theoretical and actual yield.
Calculate % yield.
Homework:
Limiting and % Yield worksheets.

29. Theoretical vs. Actual Yield of Products
Theoretical yield: maximum amount that can be produced according to the limiting reactant. (calculated yield)
Actual yield: actual amount produced in the lab.

30. Stoichiometry: Limiting Reactant
Limiting Reactant: Al
Theoretical Yield of AlCl3: moles
Limiting Reactant: C2H4
Theoretical yield of H2O: 5.4 moles
Limiting Reactant: N2
Theoretical yield of NH3: 34 g

31. Limiting Reactant

32. Stoichiometry: Percent Yield
4. Theoretical Yield of AlCl3: moles
Actual yield from lab of AlCl3: 2.8 mole
% Yield of AlCl3 :
5. Theoretical yield of H2O: 5.4 moles
Actual yield from lab of H2O: 4.9 moles
% Yield of H2O:
Theoretical yield of NH3: 34 g
Actual yield from lab of NH3: g
% yield of NH3:

33. Stoichiometry: Percent Yield
% Yield of Product: Accuracy of product formation in the lab. % Yield of product: actual yield x 100 theoretical yield Actual yield: actual amount formed in lab Theoretical yield: maximum amount that can be produced according to the limiting reactant. (calculated yield)

34. Pre-AP Chemistry (4/29) Objectives:
Identify and apply limiting reactants in a chemical equation.
Calculate percent yield of products in a chemical equation.
Identify what molarity is.
Homework:
Complete Limiting and % Yield worksheet.
Read over lab and complete hypothesis section.
*Quiz: Wednesday over stoichiometry, limiting reactants, and percent yield of products.

35. Bell Ringer: Limiting Reactants and % Yield
C2H O2 --- CO H2O
1. Balance the equation if needed.
If moles of C2H2 reacts with 7.40 moles of O2 how many grams of water can be produced?
What is the limiting reactant?
Use limiting reactant to calculate theoretical yield of H2O in grams.
If the actual yield of H2O in the lab was 40.1 grams, calculate what the % yield of H2O would be.

36. Stoichiometry Objectives: Identify what stoichiometry is in chemistry.
Apply stoichiometry calculations in chemical reactions.
Identify and apply limiting reagents in chemical reactions.
Calculate % yield of products in a chemical reaction.