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Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the KMnO4 while stirring. 1. What do you observe? 2. Why is adding slowly better? 3. How could you measure the resulting precip?

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Page 1: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

Launching Activity

1. Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3.

2. Slowly pour the NaHSO3 into the KMnO4 while stirring.

1. What do you observe?

2. Why is adding slowly better?

3. How could you measure the resulting precip?

Page 2: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

UEQ

• How does a pharmaceutical chemist know many pills it can get from a given amount of reagents?

Page 3: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

Chapter 12: Stoichiometry

Definition: Measurement of the amount of a substance in a chemical reaction.

Page 4: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

LEQ

• How is the mass relationship of a chemical reaction confirmed by the law of Conservation of Mass?

Page 5: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

• *Key: A good balanced chemical equation.*

• The Law of the Conservation of Mass applies: You must have the same before and after a reaction. ‘ The same by: mass, type of atoms, volume, and moles.

Page 6: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

Conversion factors:• 1 mole atoms = gam (gram atomic mass)

• 1 mole molecule = gmm (gram molecular mass)

• 1 mole compound = gfm (gram formula mass)

• 1 mole of any gas @ STP = 22.4 L

1 mole of anything Avogadro’s Number mass

Page 7: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

Type of stoichiometric relationships

1. Mole-mole relationships:

ie: How many moles of water are produced when 0.5 moles of oxygen react in an excess of hydrogen?

a. Write a good balanced equation.

b. From the balanced equation, write the molar ratio linking the known

to the unknown in the question.

Page 8: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

From the above question, how much hydrogen gas is left after the reaction?

**NOTE: From the balanced equation, link by the molar ratio the known to the unknown.

**NOTE: Oxygen is called the ‘limiting reactant’ b/c it will be used up before the other reactants are used.

TPS: Practice Problem #1-2 page 371 and #’s 3-4 page 372. #’s 36,40, and 41 page 392.

Page 9: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

2. Mass-mass Relationships:

mass known moles known moles unknown mass unknown

mass-mole conversion molar ratio mole-mass conversion

ie: How many grams of water is produced when 4.5 g of hydrogen reacts in an excess of oxygen?

Write a good balance equation

Convert following the flow chart.

Page 10: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

Mass-Mass Relationships

1. Law of Conservation of Mass.

2. Mass-mass relationship based on the molar ratio of a good balanced equation.Mass know>mole know>mole unknow>mass unknow

Mass-mole : mole-mole: mole-mass

Page 11: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

3. Mass-mole or Mole-mass Relationship.

mass knownmoles known moles unknown

mass-mole conversion molar ratio

4. Mass-Number of particles (# atoms, molecules or compounds).

Use 1 mole = Avogadro’s Number (6.02 x 1023).

mass knownmoles known mole unknown#

mass-mole conversion molar ratio 6.02 x 1023

Page 12: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

5. Mass-volume and Volume-massmass known moles known mole unknown

volume

6. Volume-volumeAvagodro’s Principle states that any gas at STP will occupy the same volume of 22.4L(STP = Standard Temperature and Pressure)(STP = 0oC and 1 atm)

volume known moles known moles unknown volume

Page 13: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

TSP Sample

When 45 g of CH4 burns, how many L of H2O will yield?

ans: 126 L

How many liters of methane gas is burned if 320 mole of O2 are present?

ans: 3584 L

Page 14: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

LEQ

• How efficient is a given chemical reaction?

Page 15: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

% yieldDefinition: comparison of the actual yield to the theoretical yield.

% yield = actual / theoretical x 100

1. Use mass relationships to find the theoretical yield

2. Experimentation determines the actual yield.

TSP: #28-29, page 387

Page 16: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

LEQ

• What defines when a chemical reaction stops?

Page 17: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

Limiting Reagent:

Limiting Reagent: The amount of product that will form is defined by the reactant of least amount.

Limiting reactant is defined through the comparison of the amount given to the molar ratio in a balanced equation.

Page 18: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

Steps in Limiting Reactant

• Always start with a balance equation.

• Using the balanced equation, compare the moles of reactants given.

• The limiting reactant will define product.

Page 19: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

TSP Sample

When 6.7 moles of sodium reacts with 3.2 moles of chlorine gas to produce sodium chloride. What is the limiting reactant and how many moles of product will form?

Write the balanced equation.

Use the molar ratio between reactants to compare the amount of reactant

required to react.To find the amount of product, the limiting reactant is used.

Page 20: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

TSP SampleGiven 80 g of Cu and 25 g of S to yield copper (I)

sulfide, what is the limiting reactant and how much product is produced (in grams)?

– Write a balanced equation.

– Find the # of moles of each reactant from the given masses.

– Determine, from the # of moles, which is the limiting reactant.

– Use the limiting reactant to determine the amount of product produced.

TSP: #23-24 page 383

Page 21: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

TSP: Sample Mole-MoleGiven: Fe2O3 + 3CO 2Fe + 3CO2

How many moles of CO is needed react with 25 formula units of Fe2O3?

ans: 75 moles

Given 2.25 moles of Fe2O3, how many moles of Fe will be produced?

ans: 4.5 moles

Page 22: Launching Activity 1.Measure 5 ml of 0.01 M KMnO4 and place in a 100 ml beaker and then measure 5 ml of 0.01 M NaHSO3. 2.Slowly pour the NaHSO3 into the

TPS Sample Mole-Mass

Given the same reaction as above:

How many g of Fe will be produced from 2.25 moles of Fe2O3?

ans: 251 g Fe

Given 5.4 g of Fe2O3, how many moles of CO2 will be produced?

ans: 0.10 moles


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