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Slide 1 of 36 Chemistry 16.3. © Copyright Pearson Prentice Hall Slide 2 of 36 Limiting Reagent and...
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Transcript of Slide 1 of 36 Chemistry 16.3. © Copyright Pearson Prentice Hall Slide 2 of 36 Limiting Reagent and...
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Slide 2 of 36
Limiting Reagent and Percent Yield
If a carpenter had two tabletops and seven table legs, he could only build one four-legged table. The number of table legs is the limiting factor in the construction of four-legged tables. Similarly, in chemistry, the amount of product made in a chemical reaction may be limited by the amount of one or more of the reactants.
12.3
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Limiting Reagent and Percent Yield >
Slide 3 of 36
Limiting and Excess Reagents
Limiting and Excess Reagents
How is the amount of product in a reaction affected by an insufficient quantity of any of the reactants?
12.3
Slide 4 of 36
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Limiting Reagent and Percent Yield > Limiting and Excess Reagents
In a chemical reaction, an insufficient quantity of any of the reactants will limit the amount of product that forms.
The limiting reagent is the reagent that determines the amount of product that can be formed by a reaction.
12.3
Slide 5 of 36
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Limiting Reagent and Percent Yield > Limiting and Excess Reagents
In the reaction of nitrogen and hydrogen, hydrogen is the limiting reagent. Nitrogen is the reagent that is not completely used up in the reaction. The reagent that is not used up is called the excess reagent.
12.3
Slide 6 of 36
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Limiting Reagent and Percent Yield > Limiting and Excess Reagents
12.3
The Chemical Equation for the Preparation of Ammonia
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Slide 7 of 36
Limiting Reagent and Percent Yield > Limiting and Excess Reagents
Animation 13
Apply the limiting reagent concept to the production of iron from iron ore.
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Slide 12 of 36
Practice Problems for Sample Problem 12.7
Problem Solving 12.25 Solve Problem 25 with the help of an interactive guided tutorial.
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Slide 17 of 36
Practice Problems for Sample Problem 12.8
Problem Solving 12.28 Solve Problem 28 with the help of an interactive guided tutorial.
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Limiting Reagent and Percent Yield >
Slide 18 of 36
Percent Yield
Percent Yield
What does the percent yield of a reaction measure?
12.3
Slide 19 of 36
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Limiting Reagent and Percent Yield > Percent Yield
The percent yield is a measure of the efficiency of a reaction carried out in the laboratory.
A batting average is actually a percent yield.
12.3
Slide 20 of 36
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Limiting Reagent and Percent Yield > Percent Yield
• The theoretical yield is the maximum amount of product that could be formed from given amounts of reactants.
• In contrast, the amount of product that actually forms when the reaction is carried out in the laboratory is called the actual yield.
12.3
Slide 21 of 36
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Limiting Reagent and Percent Yield > Percent Yield
The percent yield is the ratio of the actual yield to the theoretical yield expressed as a percent.
12.3
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Slide 26 of 36
Practice Problems for Sample Problem 12.9
Problem Solving 12.29 Solve Problem 29 with the help of an interactive guided tutorial.
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Slide 31 of 36
Practice Problems for Sample Problem 12.10
Problem Solving 12.31 Solve Problem 31 with the help of an interactive guided tutorial.
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Slide 32 of 36
Section Quiz
-or-Continue to: Launch:
Assess students’ understanding of the concepts in Section
12.3 Section Quiz.
12.3.
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Slide 33 of 36
12.3 Section Quiz.
1. In the reaction 3NO2 + H2O 2HNO3 + NO, how many grams of HNO3 can form when 1.00 g of NO2 and 2.25 g of H2O are allowed to react?
a. 0.913 g
b. 0.667 g
c. 15.7 g
d. 1.37 g
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Slide 34 of 36
12.3 Section Quiz.
2. How many grams of H2O can be formed from 24.0 g O2 and 6.00 g H2?
a. 30.0 g
b. 27.0 g
c. 54.0 g
d. 13.5 g
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Slide 35 of 36
3. Octane burns according to the following equation.
2C8H18 + 25O2 16CO2 + 18H2O
What is the percent yield if 14.6 g of CO2 are produced when 5.00 g of
C8H18 are burned?
a. 106%
b. 94.8%
c. 34.2%
d. 62.5%
12.3 Section Quiz.
© Copyright Pearson Prentice Hall
Slide 36 of 36
Limiting Reagent and Percent Yield > Concept Map 12
Solve the Concept Map with the help of an interactive guided tutorial.