Stoichiometry wk 2 Lesson Plan

Name: Sara Adamek

Class/Subject: AP Prep Chemistry

Date: March/April 31- 4, 2014

Student Objectives/Student Outcomes:Objectives AssessmentStudents will be able to covert between amounts of one substance and amounts of another.

Students will correctly identify given information, choose the correct conversion factor(s) and then solve the problem correctly.

Students will be able to explain why this skill is useful.

Stoichiometry allows you to determine yields and limiting reagents, both of which have applications in industry and research. Presumably it also boosts logical thinking and problem solving.

Students will be able to identify the limiting reagent.

Students will be able to solve stoichiometric problems and then choose the reactant that will limit the production of the product.

Content Standards: HS-PS1 Matter and its Interactions

HS-PS1-7. Use mathematical representations to support the claim that atoms, and therefore mass, are conserved during a chemical reaction. 

Materials/Resources/Technology:Stoichiometry challenge problems, stoichiometry mixed practice

Time (Review stoich)Start of Class:What is stoichiometry? (Calculations relating to finding out how much stuff is needed/will be produced)Why is it useful? (Can’t go around just dumping chemicals together.) Announce quiz on Thursday.Introduction of Lesson:Demo grams to moles and then grams to grams. Lesson Instruction:Pass out Practice problems. Do first problem with students. Release students to work. Assessment/Checks for understanding:Check for completion. Give feedback Closure/Wrap-up/Review: Round students up for exit slip explanation.

Ask them to answer the questions: If you are given a starting mass and a balanced equation how would you solve for the mass of product. There are 4 steps (five if you count solving the problem.

Materials/Resources/Technology:Baking soda, HCl, Mole and Mass Relationships lab guide

Time (Lab)Start of Class:Collect hw. Take attendance. Introduction of Lesson:Pass out Lab. Discuss procedure and safety. Lesson Instruction:Have students do the lab. Assessment/Checks for understanding:Grade lab questions for accuracy. Provide feedback. Closure/Wrap-up/Review:If there is time, gather students and discuss lab outcomes/ calculations.

Materials/Resources/Technology:

Time (Lab wrap up/ Mole : gram review) Start of Class:Take attendance. Pass back papers. Introduction of Lesson: Review key points of the lab. Lesson Instruction:Review Mass to mass calculations. Have students work on lab or review questions. Assessment/Checks for understanding:Grade lab for accuracy. Check HW for completion. Provide feedback for both. Closure/Wrap-up/Review:Exit slip. Given Al + Br2 AlBr3 and 5.4 grams of Br2 how many grams of AlBr3 are you going to end with?

Materials/Resources/Technology:

Time ( Quiz) Start of Class:Collect HW and lab. Pass back papers. Take attendanceIntroduction of Lesson:Pass out conversion quiz. Have students pick up A mole is not a Furry Rodent rubric and read when finished. Lesson Instruction:Discuss ‘A Mole is Not…Assignment’ with students. Emphasize that no class time will be given to work on it. Allow time for students to go look at past years’ projects. Answer questions about the Mole project.

Introduce Scientific notation. Assessment/Checks for understanding:Check activity for completion. Closure/Wrap-up/Review:

Materials/Resources/Technology:Extra copies of ‘A Mole is not a Furry Rodent’

Time (Field Trip with Substitute)2 min Start of Class:

Take attendance. Introduction of Lesson:Pass out the worksheet STOICHIOMETRY: Field trip pts. Instruct the students that they are to show all their work or they need to fill in the blanks provided. This will be due at the end of the hour; please collect it. Students my use their notes and other materials to work on the problems. They may not use their phones. (Unless they are using them as calculators, but the difference is pretty easy to spot.) They may talk quietly but if the conversations get off topic/ too loud feel free to require them to work silently. You can let them know up front that if they are not on topic they will have to work silently. If students finish the worksheet early they many work on their project “A Mole is not a Furry Mammal” or they may work on other homework.

They will try to pack up early and line up at the door. Try to keep them in their seats and working. Lesson Instruction:Students should work on the worksheet and then ‘A Mole is not a Furry Rodent’ projects. Assessment/Checks for understanding:Check wks for completion. Give feedback. Closure/Wrap-up/Review:Collect the stoichiometry worksheet.

STOICHIOMETRY: CHALLENGE PRACTICE Name:____________________

1. Given ____ (NH4)2Cr2O7 ___ Cr2O3 + ____ N2+ ____ H2Oa. What mass of Cr2O3 will be produced given 10.8 g (NH4)2Cr2O7?

b. What mass of N2 will be produced given 10.8 g (NH4)2Cr2O7?

c. What mass of H2O will be produced given 10.8 g (NH4)2Cr2O7?

2. Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel rocket motors. The reaction is:

Fe2O3 (s) + 2 Al (s) 2 Fe (l) + Al2O3 (s)

a. What mass of iron (III) oxide and aluminum must be used to produce 15.0 g iron?

b. What is the maximum mass of aluminum oxide that could be produced?

3. The reusable booster rockets of the U.S. space shuttle employ a mixture of aluminum and ammonium perchlorate for fuel. A possible equation for this reaction is

3 Al + NH4ClO4 Al2O3 + AlCl3 + 3NO + 6 H2Oa. What mass of NH4ClO4 should be used in the fuel mixture for every kilogram of Al?

4. One of the relatively few reactions that takes place directly between two solids at room temperature is below. In this equation, the ˖ 8 H2O indicates the presence of eight water molecules. Therefore the compound is called barium hydroxide octahydrate.

Ba(OH)2 ˖ 8 H2O + NH4SCN Ba(SCN)2 + H2O + NH3

a. Balance the equation.

b. What mass of ammonium thiocynate must be used if it is to react completely with 6.5 g barium hydroxide octahydrate?

5. Coke is an impure form of carbon that is often used in the industrial production of metals from their oxides. If a sample of coke is 95% carbon by mass, determine the mass of coke needed to react completely with 1.0 ton of copper (II) oxide. Assume the equation is

Coke + 2 CuO CO2 + 2 Cu

6. The compound cisplatin, Pt(NH3)2Cl2 has been studied extensively as an antitumor agent. It is synthesized by the following reaction

K2PtCl4 + 2 NH3 Pt(NH3)2Cl2 + 2KCla. What mass of cisplatin can be made from 100. g of K2PtCl4 and sufficient NH3?

b. What mass of KCl is also produced?

7. Aspirin (C9H8O4) is synthesized by reacting salicylic acid (C7H6O3) with acetic anhydride (C4H6O3).

C7H6O3 + C4H6O3 C9H8O4 + HC2H3O2

a. What mass of acetic anhydride is needed to completely consume 1.00 x 102 g salicylic acid?

b. What is the maximum mass of aspirin (the theoretical yield) that could be produced in this reaction?

STOICHIOMETRY: MIXED PRACTICE Name:______________

1. Given the balanced equation Fe2O3 (s) + 2 Al (s) 2 Fe (l) + Al2O3 (s) and 4.5 g of Fe2O3

a. How many grams of iron will you end with?

b. How many moles of Al2O3 will you end with?

c. How many moles of Al do you need?

d. Draw a microscopic picture of reaction before it begins. Hint: what do you have BEFORE the reaction happens?

e. Draw a microscopic picture of the reaction after it is finished.

2. Given the balanced equation C7H6O3 + C4H6O3 C9H8O4 + HC2H3O2 and .97 mol C7H6O3

a. How many grams of C7H6O3 did you start with?

b. How many grams of C4H6O3 did you start with?

c. How many moles of C9H8O4 did you end with?

d. How many grams of HC2H3O2 did you end with?

e. Draw a microscopic picture of the reaction.

3. Given the balanced equation Hg (l) + Br2 (l) HgBr2 (s) and 8.56 grams of HgBr2

a. How many grams of Hg did you start with?

b. How many moles of Br2 did you start with?

c. How many moles of HgBr2 did you end with?

d. Draw a microscopic picture of the reaction.

e. Draw a macroscopic (what you would see in the lab) picture of the reaction. Make sure to use labels and show amounts.

4. Given the balanced equation 4 Al + 6 HCl 3 H2 + 2 AlCl3 and 5.97 g of Ala. How many moles of aluminum did you start with?

b. How many grams of AlCl3 can you make?

c. How many moles of HCl do you need?

d. How many grams of H2 can you make?

e. How many liters of H2 can you make?

f. Draw a microscopic picture of the reaction.

STOICHIOMETRY LAB Name: ____________________

Pre-Lab discussion:In a balanced chemical equation all reactants and products must be represented by symbols or

formulas. The total number of atoms of each element must be the same on each side of the equation to satisfy the Law of Conservation of Mass.

A calculation of the formula mass of a reactant or produce enables us to convert from grams of a particular substance taking part in a reaction to moles of that substance. The mole relationship given by the coefficients of the balance equation then allows us to calculate how many moles of the every other substance will take part in the reaction.

In this experiment, we will investigate the quantitative relationships in a reaction between sodium hydrogen carbonate (NaHCO3) and hydrochloric acid (HCl). A know mass of sodium hydrogen carbonate will be reacted with excess hydrochloric acid to produce sodium chloride, carbon dioxide and water. Knowing the mass of NaHCO3 that reacts, we can determine form the balanced equation the mass of sodium chloride that should be produced. We can compare this theoretical value with the actual experimental mass of sodium chloride produced. This experiment should aid in the understanding of the mole-mass relationships that exist in a chemical reaction and in the interpretation of a balanced chemical equation.

Pre-Lab Questions:1. Write a balanced chemical equation for this experiment. 2. How much sodium chloride will be produced if you used 2.50 g of sodium hydrogen carbonate. 3. What is the equation for figuring experimental error.

Purpose:Compare the experimental mass of a produce of a chemical reaction with the mass predicted for

that product by calculation.

Materials:Balance Microspatula Wire gauzeBurner Dropper pipet Hydrochloric acidEvaporating dish Ring Stand Sodium hydrogen carbonateWatch Glass Iron ring

Procedure:1. Record the mass of the evaporating dish and watch glass. 2. Measure out 2.50 g of NaHCO3 into your evaporating dish and record

the mass of the dish, glass and chemical. 3. Using a dropper pipet slowly add HCL to the NaHCO3 in the

evaporating dish a few drops at a time. Continuing adding acid until the reaction stops. (Make sure the watch glass is on the evaporating dish. CAUTION: HCl is a strong acid and can cause painful burns. If you get it on your skin immediately wash the area.

4. After making sure the bubbling has stopped take the watch glass off. 5. Set up the ring stand with the wire gauze and the Bunsen burner. 6. Put the evaporating dish on the set up and heat GENTLY. If it starts

to pop or spit take the flame away and put on the watch glass. 7. When all the liquid has evaporated, turn off the flame and let the dish

cool. 8. When the evaporating dish is cool find the mass of the watch glass,

evaporating dish and product. Record this number.

Data table: Evaporating dish and watch glass

Evaporating dish, watch glass and NaHCO3

Evaporating dish, watch glass and Product

Calculations:1. Find the mass of the NaHCO3 reactant. 2. Find the mass of the NaCl product.

Conclusions: 1. According the the balanced equation for the reaction, what is the ratio of moles of NaHCO3 to the

moles of NaCl? 2. How many moles of NaHCO3 are reacted in your experiment? How many moles of NaCl are

produce in your experiment? What is the ratio of moles of NaHCO3 to moles of NaCl produce in your lab?

3. In your pre-lab questions you calculated the expected mass of NaCl produced. Use this to calculate your experimental error for your experiment.

4. If all of the masses of all but one of the substances that take part in the chemical reaction are known, explain why it is possible to determine the unknown mass of the last substance.

5. In the chemical reaction CaCO3 CaO + CO2 if 40.0 g of CaCO3 are decomposed:a. How many grams of CaO are produced? b. How many grams of CO2 are produced?

6. In the reaction N2 + 3H2 2 NH3 if 20.0 g of hydrogen react:a. How many grams of ammonia are produced?b. How many grams of nitrogen react?

STOICHIOMETRY: INQUIRY LAB

When Mrs. Adamek when into the store room she discovered that the labels had fallejn off several of the containers. One of the containers had baking soda (NaHCO3) in it. Help Mrs. Adamek figure out which one is the baking soda.

Pre-Lab Discussion:

In a balanced chemical equation all reactants and products must be represented by symbols or formulas. The total number of atoms of each element must be the same on each side of the equation to satisfy the Law of Conservation of Mass.

If you know the formula mass of a reactant or product you are able to convert from grams of a particular substance taking part in a reaction to moles of that substance. The mole relationship given by the coefficients of the balanced equation then allows us to calculate how many moles of the every other substance will take part in the reaction.

In this experiment, we will compare the mass of product produced with the mass of product we would expect if the unknown was sodium hydrogen carbonate (NaHCO3). We know that NaHCO3 will react with hydrochloric acid to produce sodium chloride, water and carbon dioxide. We can compare this theoretical value with the actual experimental mass of sodium chloride produced to determine which of the unknowns is baking soda. This experiment should aid in the understanding of the mole-mass relationships that exist in a chemical reaction and in the interpretation of a balanced chemical equation.

Pre-Lab Questions:Answer these on a separate piece of paper.

1. Write a balanced chemical equation for this experiment. 2. How much sodium chloride will be produced if you used 2.50 g of sodium hydrogen carbonate? 3. What is the equation for figuring experimental error?

Materials:Balance Microspatula Wire gauzeBurner Dropper pipet Hydrochloric acidEvaporating dish Ring Stand Sodium hydrogen carbonateWatch Glass Iron ring

Procedure: 1. Record the mass of the evaporating dish and watch glass. 2. Measure out 2.50 g of unknown into your evaporating dish and record the mass of the dish, glass

and chemical. 3. Using a dropper pipet slowly add HCL to the unknown in the evaporating dish a few drops at a

time. Continuing adding acid until the reaction stops. Make sure the watch glass is on the evaporating dish. CAUTION: HCl is a strong acid and can cause painful burns. If you get it on your skin immediately wash the area.

4. After making sure the bubbling has stopped, take the watch glass off. 5. Set up the ring stand with the wire gauze and the Bunsen burner. 6. Put the evaporating dish on the set up and heat GENTLY. If it starts to pop or spit take the flame

away and put on the watch glass. Let it cool for a minute and then start heating again. 7. When all the liquid has evaporated, turn off the flame and let the dish cool. 8. When the evaporating dish is cool find the mass of the watch glass, evaporating dish and product.

Record this number. 9. Wash the evaporating dish and watch glass with soap and water. The product may go down the

drain. Put away the rest of your materials.

Data table: Unknown A

Evaporating dish and watch glass

Evaporating dish, watch glass and Unknown A

Evaporating dish, watch glass and Product

Unknown BEvaporating dish and watch glass

Evaporating dish, watch glass and Unknown B

Evaporating dish, watch glass and Product

Calculations:Do these on a separate piece of paper.

1. Find the mass of each of the unknown reactants. 2. Calculate the expected (theoretical) amount of product based on the mass

of the unknown. Assume the unknown is baking soda. 3. Find the masses of each of the products. 4. Calculate the percent error for each unknown.

Conclusions: Please answer in complete sentences on a separate piece of paper. 1. According to the balanced equation for the reaction, what is the ratio of moles of NaHCO3 to

the moles of NaCl? (2 pts)2. Which of the unknowns is baking soda? How did you know? (6pts) 3. If your percent error was greater than zero describe some sources of error. (2 pts)

DUE Friday, April 18thYour task:

1. You must create an original visual display (i.e. poster, pamphlet, PowerPoint, video etc) that illustrates the concept of a mole.

2. You must create a visual/written explanation (step-by-step) of how to solve a stoichiometric mole problem

The following must be included:1. The definition of a mole. 2. A balanced chemical equation. You may reproduce one from a lab or text, but you must cite the

place from which you obtained it.3. An original word problem based on the balanced equation. The problem can be a mass-mass,

mass-volume, or a volume-volume problem. You will earn more points by choosing a harder problem. Mass-mass and mass-volume problems are typically more involved and more difficult. Ratios of moles that are not 1:1 or 1:2 are also more difficult.

4. A step-by-step solution that is clearly set up, illustrated, and explained with captions, etc. 5. Your work must be of the highest quality. Examples of quality work will be shown.

Additional Information:1. You may work alone or with one partner. (A video may have more than 2, but everyone must

have a CLEARLY DEFINED ROLE in producing the video). You must sign up for a group in the next two days. If you do not sign up for a group you will have to do the project on your own.

2. All work on the project will be done outside of class. Therefore, if you work in a group, choose people who you can get together with easily.

3. Your project is worth 40 points (as a test grade) and will be graded according to the rubric below.

Accuracy Thoroughness & Clarity Complexity Visual Display10 pts

The written and visual displays are free of any math, molar conversion or unit errors.

The description of how molar conversions are used is logical and thorough. Complete and logical sentences describe the work.

The stoichiometric problem is a mass-mass or volume-mass problem with uneven rations (2:5, 3:5 3:4 etc)

The diagram is well organized, neatly displayed and visually pleasing.

9 pts

There are one or two minor errors that are basically inconsequential.

The descriptions are logical and through enough to be understandable by the reader.

The stoichiometric problem is a mass-mass or volume-mass problem with uneven rations (2:5, 3:5 3:4 etc)

The diagrams are readable and organized but not as clearly detailed or visually pleasing.

8 pts

One major math, molar conversion or unit error may be present, but the majority of the work is correct.

The descriptions are incomplete or illogical to the reader, but are correct upon questioning.

The stoichiometric problem is a mass-mass, or volume-mass problem with simple ratios (ex. 1:1 or 1:2)

The diagrams are somewhat difficult to read or follow. Overall format is sloppy.

≤ 7 pts

Several major math, molar conversion, or unit errors exist.

The descriptions are incomplete and illogical.

The stoichiometric problem is a mole-mole or volume-volume problem or the ratios are simple.

Major flaws in organization and diagrams are incomplete or unclear.

STOICHIOMETRY QUIZ Name: ____________________

Show all your work!

1. Calculate the number of grams of H2 that can be produced from 6.80 g of aluminum. (4pts)

2 Al + 6 NaOH 2 Na3AlO3 + 3 H2

2. How many grams of iron (III) oxide can be obtained by heating 975 g of iron (II) sulfide? (4pts)

4 FeS + 7 O2 2 Fe2O3 + 4 SO2

3. Calculate the number of grams of water that could be produced from the burning of 51 g of ethane (C2H6). (5pts)

___ C2H6 + ___ O2 ___ CO2 + ____H2O (unbalanced)

4. Draw a microscopic picture of the reaction in problem 1. (2pts)

STOICHIOMETRY: Scientific Notation Challenge Name:_________________

1. How many grams of LiCl does it take to react with 1.0 g of Pb(NO3)2?Pb(NO3)2 + 2 LiCl 2 LiNO3 + PbCl2

2. 51.0g of NH3 are reacted according to the following equation:2 NH3 3 H2 + N2

a. How many liters of H2 are produced?b. How many liters of N2 are produced? c. How many molecules of N2 are produced?

3. How many molecules of H2O will be made when 5.0 x 1024 molecules of H2 are reacted with excess O2.

4. 20 molecules of calcium chloride reacts with excess silver nitrate to create calcium nitrate and silver chloride. How many moles of silver chloride will be produced?

5. Given HCl + NaOH H2O + NaCla. How many liters of H2O gas will be made from 500 grams of HCl? b. How many liters of H2O will be made from 500 grams of NaOH?c. Which produces more?

6. If 10 moles of pentane, C5H12, are burned, how many molecules of CO2 will be produced?

7. If 0.2 L of methane (CH4) gas is burned. How many moles of CO2 will be produced?

8. How many grams of propane (C3H8) need to be burned if you want to produce 0.10 L of water vapor (a gas) at STP?

9. How many grams of PCl3 will be produced when 1.43 x 1020 molecules of PCl5 are reacted?PCl5 PCl3 + Cl

10. In the Bish process, water is created from HI and Ca(OH)2 according to the reaction below. 2 HI + Ca(OH) CaI2 + 2H2O

The water is then used to react with CO2 to create octane and oxygen.18 H2O + 16 CO2 2 C8H18 + 25 O2

How many molecules of octane can be created from 250 g of Ca(OH)2?

STOICHIOMETRY: Scientific Notation Practice Name:_________________

Put all of your answers into scientific notation.

1. How many grams of PCl3 will be produced when 90 moles of PCl5 are reacted?PCl5 PCl3 + Cl

2. How many grams of LiCl does it take to react with 1.0 g of Pb(NO3)2?Pb(NO3)2 + 2 LiCl 2 LiNO3 + PbCl2

3. 51.0g of NH3 are reacted according to the following equation:2 NH3 3 H2 + N2

d. How many liters of H2 are produced?e. How many liters of N2 are produced? f. How many molecules of N2 are produced?

4. How many liters of H2O will be made when 50 moles of H2 are reacted with excess O2?

5. 0.13 g of calcium chloride reacts with excess silver nitrate to create calcium nitrate and silver chloride.

a. Write a balanced equation for this reaction. b. How many moles of silver chloride will be produced?

6. Given HCl + NaOH H2O + NaCla. How many liters of H2O gas will be made from 500 grams of HCl? b. How many liters of H2O will be made from 500 grams of NaOH?c. Which reactant produces more product?

7. If 10 moles of pentane, C5H12, are burned, how many liters of CO2 will be produced? C5H12 + 8 O2 6 H2O + 5 CO2

8. If 0.20 L of methane (CH4) gas is burned, how many moles of CO2 will be produced? CH4 + 2 O2 2 H2O + CO2

9. How many grams of propane (C3H8) need to be burned if you want to produce 0.1 L of water vapor (a gas) at STP?

C3H8 + 5 O2 4 H2O + 3 CO2

10. How many grams of HI did you start with if you end with 0.1 g CaI2? 2 HI + Ca(OH) CaI2 + 2H2O

STOICHIOMETRY: Field trip pts Name: _____________________1. How many grams of hydrogen are produced when 67.12 g of HCl are reacted with copper?

2 HCl + Cu CuCl2 + H2

2. How many moles of oxygen are produce in the decomposition reaction of 145. 73 g of sodium chlorate?

2 NaClO3 2 NaCl + 3 O2

3. 98.03 g of magnesium hydroxide are decomposed in the reaction below. How many grams of water are produced?

Mg(OH)2 MgO + H2O

4. How many grams of lead (II) nitrate are needed to produce 49.23 g of sodium nitrate? Pb(NO3)2 + 2 NaCl PbCl2 + 2 NaNO3

5. How many moles of silver are produced when 36.92 grams of copper displaces silver from silver nitrate in the reaction below?

___Cu + ___ AgNO3 ___Ag + ____Cu(NO3)2

6. HCl is reacted with CaCO3 to produce 7.45 moles of CO2. How many grams of hydrochloric acid were needed to produce this amount of CO2?

____HCl + ____CaCO3 ____CO2 + ____CaCl2

7. If 42.84 grams of iron are reacted with water, how many grams of iron(III) oxide are produced? ____Fe + ____H2O ____Fe2O3 +____ H2

8. How many grams of aluminum hydroxide are produced if 165.7 g of aluminum sulfate are reacted with calcium hydroxide.

____ Al2(SO4)3 + ____ Ca(OH)2 ____Al(OH)3 + ____CaSO4

9. In this synthesis reaction below, 29.48 g of fluorine are reacted with excess sodium. How many moles of NaF are produced?

___ Na + ___ F2 ____ NaF

10. If 8.4 moles of aluminum bromide is reacted with fluorine, how many grams of bromine are produced?

___F2 +___ AlBr3 ____Br2 + ____AlF3