Chemistry 16.3
Limiting Reagent and Percent Yield <ul><li>If a carpenter had two tabletops and seven table legs, he could only build one ...
Limiting and Excess Reagents <ul><li>Limiting and Excess Reagents </li></ul><ul><ul><li>How is the amount of product in a ...
Limiting and Excess Reagents <ul><ul><ul><li>In a chemical reaction, an insufficient quantity of any of the reactants will...
Limiting and Excess Reagents <ul><ul><ul><li>In the reaction of nitrogen and hydrogen, hydrogen is the limiting reagent. N...
Limiting and Excess Reagents 12.3 The Chemical Equation for the Preparation of Ammonia
Limiting and Excess Reagents <ul><ul><li>Animation 13   </li></ul></ul><ul><ul><li>Apply the limiting reagent concept to t...
12.7
12.7
12.7
12.7
for Sample Problem 12.7 Problem Solving 12.25  Solve Problem 25 with the help of an interactive guided tutorial.
12.8
12.8
12.8
12.8
for Sample Problem 12.8 Problem Solving 12.28  Solve Problem 28 with the help of an interactive guided tutorial.
Percent Yield <ul><li>Percent Yield </li></ul><ul><ul><li>What does the percent yield of a reaction measure? </li></ul></u...
Percent Yield <ul><ul><ul><li>The percent yield is a measure of the efficiency of a reaction carried out in the laboratory...
Percent Yield <ul><ul><ul><ul><li>The  theoretical yield  is the maximum amount of product that could be formed from given...
Percent Yield <ul><ul><ul><li>The  percent yield  is the ratio of the actual yield to the theoretical yield expressed as a...
12.9
12.9
12.9
12.9
for Sample Problem 12.9 Problem Solving 12.29  Solve Problem 29 with the help of an interactive guided tutorial.
12.10
12.10
12.10
12.10
for Sample Problem 12.10 Problem Solving 12.31  Solve Problem 31 with the help of an interactive guided tutorial.
12.3 Section Quiz. <ul><li>12.3. </li></ul>
12.3  Section Quiz. <ul><ul><li>1. In the reaction 3NO 2  + H 2 O    2HNO 3  + NO, how many grams of HNO 3  can form when...
12.3  Section Quiz. <ul><ul><li>2. How many grams of H 2 O can be formed from 24.0 g O 2  and 6.00 g H 2 ? </li></ul></ul>...
<ul><ul><li>3. Octane burns according to the following equation.  </li></ul></ul><ul><ul><li>2C 8 H 18  + 25O 2    16CO 2...
Concept Map 12 <ul><ul><li>Solve the Concept Map with the help of an interactive guided tutorial. </li></ul></ul>
<ul><li>END OF SHOW </li></ul>
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Chapter12 Section03 Edit

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  • Chapter12 Section03 Edit

    1. 1. Chemistry 16.3
    2. 2. Limiting Reagent and Percent Yield <ul><li>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. </li></ul>12.3
    3. 3. Limiting and Excess Reagents <ul><li>Limiting and Excess Reagents </li></ul><ul><ul><li>How is the amount of product in a reaction affected by an insufficient quantity of any of the reactants? </li></ul></ul>12.3
    4. 4. Limiting and Excess Reagents <ul><ul><ul><li>In a chemical reaction, an insufficient quantity of any of the reactants will limit the amount of product that forms. </li></ul></ul></ul><ul><ul><ul><ul><li>The limiting reagent is the reagent that determines the amount of product that can be formed by a reaction. </li></ul></ul></ul></ul>12.3
    5. 5. Limiting and Excess Reagents <ul><ul><ul><li>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. </li></ul></ul></ul>12.3
    6. 6. Limiting and Excess Reagents 12.3 The Chemical Equation for the Preparation of Ammonia
    7. 7. Limiting and Excess Reagents <ul><ul><li>Animation 13 </li></ul></ul><ul><ul><li>Apply the limiting reagent concept to the production of iron from iron ore. </li></ul></ul>
    8. 8. 12.7
    9. 9. 12.7
    10. 10. 12.7
    11. 11. 12.7
    12. 12. for Sample Problem 12.7 Problem Solving 12.25 Solve Problem 25 with the help of an interactive guided tutorial.
    13. 13. 12.8
    14. 14. 12.8
    15. 15. 12.8
    16. 16. 12.8
    17. 17. for Sample Problem 12.8 Problem Solving 12.28 Solve Problem 28 with the help of an interactive guided tutorial.
    18. 18. Percent Yield <ul><li>Percent Yield </li></ul><ul><ul><li>What does the percent yield of a reaction measure? </li></ul></ul>12.3
    19. 19. Percent Yield <ul><ul><ul><li>The percent yield is a measure of the efficiency of a reaction carried out in the laboratory. </li></ul></ul></ul><ul><ul><ul><li>A batting average is actually a percent yield. </li></ul></ul></ul>12.3
    20. 20. Percent Yield <ul><ul><ul><ul><li>The theoretical yield is the maximum amount of product that could be formed from given amounts of reactants. </li></ul></ul></ul></ul><ul><ul><ul><ul><li>In contrast, the amount of product that actually forms when the reaction is carried out in the laboratory is called the actual yield . </li></ul></ul></ul></ul>12.3
    21. 21. Percent Yield <ul><ul><ul><li>The percent yield is the ratio of the actual yield to the theoretical yield expressed as a percent. </li></ul></ul></ul>12.3
    22. 22. 12.9
    23. 23. 12.9
    24. 24. 12.9
    25. 25. 12.9
    26. 26. for Sample Problem 12.9 Problem Solving 12.29 Solve Problem 29 with the help of an interactive guided tutorial.
    27. 27. 12.10
    28. 28. 12.10
    29. 29. 12.10
    30. 30. 12.10
    31. 31. for Sample Problem 12.10 Problem Solving 12.31 Solve Problem 31 with the help of an interactive guided tutorial.
    32. 32. 12.3 Section Quiz. <ul><li>12.3. </li></ul>
    33. 33. 12.3 Section Quiz. <ul><ul><li>1. In the reaction 3NO 2 + H 2 O  2HNO 3 + NO, how many grams of HNO 3 can form when 1.00 g of NO 2 and 2.25 g of H 2 O are allowed to react? </li></ul></ul><ul><ul><ul><li>0.913 g </li></ul></ul></ul><ul><ul><ul><li>0.667 g </li></ul></ul></ul><ul><ul><ul><li>15.7 g </li></ul></ul></ul><ul><ul><ul><li>1.37 g </li></ul></ul></ul>
    34. 34. 12.3 Section Quiz. <ul><ul><li>2. How many grams of H 2 O can be formed from 24.0 g O 2 and 6.00 g H 2 ? </li></ul></ul><ul><ul><ul><li>30.0 g </li></ul></ul></ul><ul><ul><ul><li>27.0 g </li></ul></ul></ul><ul><ul><ul><li>54.0 g </li></ul></ul></ul><ul><ul><ul><li>13.5 g </li></ul></ul></ul>
    35. 35. <ul><ul><li>3. Octane burns according to the following equation. </li></ul></ul><ul><ul><li>2C 8 H 18 + 25O 2  16CO 2 + 18H 2 O </li></ul></ul><ul><ul><li>What is the percent yield if 14.6 g of CO 2 are produced when 5.00 g of C 8 H 18 are burned? </li></ul></ul><ul><ul><ul><li>106% </li></ul></ul></ul><ul><ul><ul><li>94.8% </li></ul></ul></ul><ul><ul><ul><li>34.2% </li></ul></ul></ul><ul><ul><ul><li>62.5% </li></ul></ul></ul>12.3 Section Quiz.
    36. 36. Concept Map 12 <ul><ul><li>Solve the Concept Map with the help of an interactive guided tutorial. </li></ul></ul>
    37. 37. <ul><li>END OF SHOW </li></ul>

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