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

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Presentation on theme: "Chemistry (4/25) Objectives: Complete Chemical Quantities Exam Perform Hydrate Lab Homework: Answer post lab questions."— Presentation transcript:

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(SO 4 ). H 2 O ----> Cu(SO 4 ) + H 2 O Post-Lab questions: Use the equation above to help answer the following questions: 1.What was the hydrate salt in this experiment? 2.What was the anhydrous salt in this experiment? 3.What was the difference between the hydrated salt and the anhydrous salt in this experiment? 4.Was this a physical or chemical reaction? Validate your answer with data from your lab.

5 Hydrate Lab Cu(SO 4 ). H 2 O ----> Cu(SO 4 ) + H 2 O

6 Copper Sulfate Hydrate

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

8 Stoichiometry N 2 + 3H > 2NH 3 (NH 3 ) (N 2 )

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 1.Calculate the percent composition of water in this hydrate: Mg(SO 4 ). 7H 2 O (Epsom Salt) 2.What is stoichiometry? 3. N 2 H 4 + O > N 2 + H 2 O a. Balance the chemical equation. b. How many moles of rocket fuel (N 2 H 4 ) are needed to produce 8 moles of N 2 ?

11 Bell Ringer 1.Calculate the percent composition of water in this hydrate: Mg(SO 4 ). 7H 2 O (Epsom Salt) 2.What is stoichiometry? 3. N 2 H 4 + O > N 2 + H 2 O a. Balance the chemical equation. b. How many moles of rocket fuel (N 2 H 4 ) are needed to produce 8 moles of N 2 ?

12 Bell Ringer 1.Calculate the percent composition of water in this hydrate: Mg(SO 4 ). 7H 2 O (Epsom Salt) 2.What is stoichiometry? 3. N 2 H 4 + O > N 2 + H 2 O a. Balance the chemical equation. b. How many moles of rocket fuel (N 2 H 4 ) are needed to produce 8 moles of N 2 ?

13 Stoichiometry N 2 + 3H > 2NH 3 Stoichiometry: Converting between substances in a balanced chemical equation using mole conversions. (NH 3 ) (N 2 )

14 Stoichiometry H 2 O > H 2 + O 2 1.What type of reaction is this? 2.Balance the chemical equation if needed. 3.If you start with 100 moles of H 2 O how many moles of H 2 would be produced? 3.If you want to produce 3.8moles of O 2, how much H 2 O 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 N 2 + 3H > 2NH 3 Stoichiometry: Converting between substances in a balanced chemical equation using mole conversions.

18 Stoichiometry Problems N 2 H 4 + O > N H 2 O If 13.8 grams of water were produced how much rocket fuel (N 2 H 4 ) 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 N 2 + 3H > 2NH 3 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 N 2 + 3H > 2NH 3 Stoichiometry: Converting between substances in a balanced chemical equation using mole conversions.

24 Stoichiometry: Limiting Reactants Limiting Reactant: 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 2 + H 2 1.What type of reactions is this? 2.Balance equation if needed. 3.If 6.8 moles of Mg react with 7.5 moles of HCl which is considered the limiting reactant? excess reactant? ReactantsHave (moles)Need (moles)

27 Stoichiometry: Limiting Reactant 2HCl + Mg > MgCl 2 + H 2 1.If 6.8 moles of Mg react with 7.5 moles of HCl how many moles of MgCl 2 can be produced? ReactantsHave (moles)Need (moles) HCl (limited)7.5 mol13.6 Mg (excess)6.8 mol3.75

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 4.Limiting Reactant: Al Theoretical Yield of AlCl 3 : 3.0 moles 5.Limiting Reactant: C 2 H 4 Theoretical yield of H 2 O: 5.4 moles 6.Limiting Reactant: N 2 Theoretical yield of NH 3 : 34 g

31 Limiting Reactant

32 Stoichiometry: Percent Yield 4. Theoretical Yield of AlCl 3 : 3.0 moles Actual yield from lab of AlCl 3 : 2.8 mole % Yield of AlCl 3 : 5. Theoretical yield of H 2 O: 5.4 moles Actual yield from lab of H 2 O: 4.9 moles % Yield of H 2 O: 6.Theoretical yield of NH 3 : 34 g Actual yield from lab of NH 3 : 31.5 g % yield of NH 3 :

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 C 2 H 2 + O  CO 2 + H 2 O 1. Balance the equation if needed. 2.If 2.40 moles of C 2 H 2 reacts with 7.40 moles of O 2 how many grams of water can be produced? a.What is the limiting reactant? b.Use limiting reactant to calculate theoretical yield of H 2 O in grams. c.If the actual yield of H 2 O in the lab was 40.1 grams, calculate what the % yield of H 2 O 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.


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