Reinforced S.15.C.6 Identify the physical state for each substance in a reaction equation Reinforced Chapter menu Resources Copyright © by Holt, Rinehart and Winston.
Download ReportTranscript Reinforced S.15.C.6 Identify the physical state for each substance in a reaction equation Reinforced Chapter menu Resources Copyright © by Holt, Rinehart and Winston.
Reinforced S.15.C.6 Identify the physical state for each substance in a reaction equation Reinforced Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved.
Main Standards Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved.
Chapter 9
Table of Contents Stoichiometry Section 3 Limiting Reactants and Percentage Yield Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved.
Chapter 9
Section 3 Limiting Reactants and Percentage Yield Objectives • Describe a method for determining which of two reactants is a limiting reactant.
• Calculate the amount in moles or mass in grams of a product, given the amounts in moles or masses in grams of two reactants, one of which is in excess.
• Distinguish between theoretical yield, actual yield, and percentage yield.
• Calculate percentage yield, given the actual yield and quantity of a reactant.
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Chapter 9
Section 3 Limiting Reactants and Percentage Yield Limiting Reactants • The limiting reactant is the reactant that limits the amount of the other reactant that can combine and the amount of product that can form in a chemical reaction. • The excess reactant is the substance that is not used up completely in a reaction.
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Chapter 9
Visual Concepts Limiting Reactants and Excess Reactants Click below to watch the Visual Concept.
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Chapter 9
Section 3 Limiting Reactants and Percentage Yield Limited Reactants, continued Sample Problem F Silicon dioxide (quartz) is usually quite unreactive but reacts readily with hydrogen fluoride according to the following equation.
SiO 2 (s) + 4HF(g) SiF 4 (g) + 2H 2 O(l) If 6.0 mol HF is added to 4.5 mol SiO 2 , which is the limiting reactant?
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Chapter 9
Section 3 Limiting Reactants and Percentage Yield Limited Reactants, continued Sample Problem F Solution SiO 2 (s) + 4HF(g) SiF 4 (g) + 2H 2 O(l) Given: amount of HF = 6.0 mol amount of SiO 2 = 4.5 mol Unknown: limiting reactant mole ratio Solution: mol HF mol SiF 4 mol HF mol SiF 4 produced mol SiO 2 mol SiF 4 mol SiO 2 mol SiF 4 produced Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved.
Chapter 9
Section 3 Limiting Reactants and Percentage Yield Limited Reactants, continued Sample Problem F Solution, continued SiO 2 (s) + 4HF(g) SiF 4 (g) + 2H 2 O(l) 6.0
mol HF 1 mol SiF 4 4 mol HF 1.5
mol SiF 4 produced 4.5
mol SiO 2 1 mol SiF 4 1 mol SiO 2 4.5
mol SiF 4 produced HF is the limiting reactant.
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Chapter 9
Practice Problems p.313
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Chapter 9
ANSWERS Practice Problems p.313
Make sure you understand why.
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Chapter 9
Complete all of these Practice Problems p.315
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Chapter 9
ANSWERS Practice Problems p.315
Make sure you understand why.
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Chapter 9
Section 3 Limiting Reactants and Percentage Yield Percentage Yield • • The theoretical yield is the maximum amount of product that can be produced from a given amount of reactant.
• The actual yield of a product is the measured amount of that product obtained from a reaction.
The percentage yield is the ratio of the actual yield to the theoretical yield, multiplied by 100.
percentage yield actual yield theorectical yield 100 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved.
Chapter 9
Visual Concepts Comparing Actual and Theoretical Yield Click below to watch the Visual Concept.
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Chapter 9
Percent Yield Visual Concept Click below to watch the Visual Concept.
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Chapter 9
Section 3 Limiting Reactants and Percentage Yield Percentage Yield, continued Sample Problem H Chlorobenzene, C 6 H 5 Cl, is used in the production of many important chemicals, such as aspirin, dyes, and disinfectants. One industrial method of preparing chlorobenzene is to react benzene, C 6 H 6 , with chlorine, as represented by the following equation.
C 6 H 6 (l) + Cl 2 (g) C 6 H 5 Cl(l) + HCl(g) When 36.8 g C 6 H 6 react with an excess of Cl 2 , the actual yield of C 6 H 5 Cl is 38.8 g.
What is the percentage yield of C 6 H 5 Cl?
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Chapter 9
Section 3 Limiting Reactants and Percentage Yield Percentage Yield, continued Sample Problem H Solution Given: C 6 H 6 (l) + Cl 2 (g) C 6 H 5 Cl(l) + HCl(g) mass of C 6 H 6 = 36.8 g mass of Cl 2 = excess Unknown: actual yield of C 6 H 5 Cl = 38.8 g percentage yield of C 6 H 5 Cl Solution: Theoretical yield molar mass factor mol ratio molar mass g C 6 H 6 mol C 6 H 6 g C 6 H 6 mol C 6 H 5 Cl mol C 6 H 6 g C 6 H 5 Cl mol C 6 H 5 Cl g C 6 H 5 Cl Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved.
Chapter 9
Section 3 Limiting Reactants and Percentage Yield Percentage Yield, continued Sample Problem H Solution, continued C 6 H 6 (l) + Cl 2 (g) C 6 H 5 Cl(l) + HCl(g) Theoretical yield 36.8
g C 6 H 6 1 mol C 6 H 6 78.12
g C 6 H 6 Percentage yield 53.0
g C 1 6 1 mol H 5 mol Cl C 6 C H 6 5 H Cl 6 actual yield percentage yield C 6 H 5 Cl 112.56
g C 6 H 5 Cl theorectical yield 1 mol C 6 H 5 Cl 100 percentage yield 38.8
g 53.0
g 100 73.2% Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved.
Chapter 9
Practice Problems pg. 318
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Chapter 9
ANSWERS - Practice Problems pg. 318
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Online Self-Check Quiz
Complete the online Quiz and record answers. Ask if you have any questions about your answers. click here for online Quiz 9.3
(7 questions) You must be in the “Play mode” for the slideshow for hyperlink to work.
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Chapter 9
LIMITING REACTANT PROBLEM ACTIVITY Click below to watch the PROBLEM ACTIVITY.
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Chapter 9
LIMITING REACTANTS PROBLEM ACTIVITY Click below to watch the PROBLEM ACTIVITY.
LIMITING REACTANTS Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved.
Chapter 9
Percent Yield PROBLEM ACTIVITY Click below to watch the PERCENT YIELD PROBLEM.
PERCENT YIELD Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved.
VIDEOS FOR ADDITIONAL INSTRUCTION
Additional Videos for Section 9.3: Limiting Reactants and Percent Yield Percent Yield Limiting Reactants © Copyright Pearson Prentice Hall Slide of 28 End Show
SCI LINKS FOR CHAPTER
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