chapter 9 lecture basic chemistry fourth edition 9.4 percent yield learning goal given the actual...
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![Page 1: Chapter 9 Lecture Basic Chemistry Fourth Edition 9.4 Percent Yield Learning Goal Given the actual quantity of product, determine the percent yield for](https://reader035.vdocument.in/reader035/viewer/2022062217/5697c0251a28abf838cd553f/html5/thumbnails/1.jpg)
Chapter 9 Lecture
Basic ChemistryFourth Edition
9.4 Percent Yield
Learning Goal Given the actual quantity of product, determine the percent yield for a reaction.
© 2014 Pearson Education, Inc.
Chapter 9 Chemical Quantities in Reactions
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Theoretical yield is the amount of product we expect, if all the reactants were converted to the desired product.
Actual yield is the amount of product obtained when the reaction takes place.
Percent yield is the ratio of actual yield to theoretical yield.
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Percent Yield
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On a space shuttle, LiOH is used to absorb exhaled CO2 and form LiHCO3.
LiOH(s) + CO2(g) LiHCO3(s)
Calculating Percent Yield
On a space shuttle, the LiOH in the canisters removes Co2 from the air.
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Calculating Percent Yield
What is the percent yield of LiHCO3 if 50.0 g of LiOH produces 72.8 g of LiHCO3?
LiOH(s) + CO2(g) LiHCO3(s)
Step 1 State the given and needed quantities. Given: 50.0 g of LiOH,
72.8 g of LiHCO3
Need: Theoretical yield, LiHCO3 Percent yield, LiHCO3
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LiOH(s) + CO2(g) LiHCO3(s)
50.0 g 72.8 g Actual yield? Theoretical yield
Step 2 Write a plan to calculate the theoretical and percent yield.
Calculating Percent Yield
grams of LiOH
Molar MassMolar Mass
moles ofLiOH
Molar MassMolar Mass
moles of LiHCO3
grams ofLiHCO3
Mole–Mole factor
Mole–Mole factor
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LiOH(s) + CO2(g) LiHCO3(s)
50.0 g 72.8 g Actual yield? Theoretical yield
Step 3 Write the molar mass and mole−mole factors.
1 mole of LiOH = 23.95 g of LiOH
Calculating Percent Yield
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LiOH(s) + CO2(g) LiHCO3(s)
50.0 g 72.8 g Actual yield? Theoretical yield
Step 3 Write the molar mass and mole−mole factors.
1 mole of LiHCO3 = 67.96 g of LiHCO3
Calculating Percent Yield
![Page 8: Chapter 9 Lecture Basic Chemistry Fourth Edition 9.4 Percent Yield Learning Goal Given the actual quantity of product, determine the percent yield for](https://reader035.vdocument.in/reader035/viewer/2022062217/5697c0251a28abf838cd553f/html5/thumbnails/8.jpg)
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LiOH(s) + CO2(g) LiHCO3(s)
50.0 g 72.8 g Actual yield ? Theoretical yield
Step 3 Write the molar mass and mole−mole factors.
1 mole of LiOH = 1 mole of LiHCO3
Calculating Percent Yield
![Page 9: Chapter 9 Lecture Basic Chemistry Fourth Edition 9.4 Percent Yield Learning Goal Given the actual quantity of product, determine the percent yield for](https://reader035.vdocument.in/reader035/viewer/2022062217/5697c0251a28abf838cd553f/html5/thumbnails/9.jpg)
© 2014 Pearson Education, Inc.
Calculating Percent Yield
LiOH(s) + CO2(g) LiHCO3(s)
50.0 g 72.8 g Actual yield? Theoretical yield
Step 4 Calculate the percent yield by dividing the actual yield by the theoretical yield and multiplying by 100%. Calculation of theoretical yield:
![Page 10: Chapter 9 Lecture Basic Chemistry Fourth Edition 9.4 Percent Yield Learning Goal Given the actual quantity of product, determine the percent yield for](https://reader035.vdocument.in/reader035/viewer/2022062217/5697c0251a28abf838cd553f/html5/thumbnails/10.jpg)
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Calculating Percent Yield
LiOH(s) + CO2(g) LiHCO3(s)
50.0 g 72.8 g Actual yield ? Theoretical yield
Step 4 Calculate the percent yield by dividing the actual yield by the theoretical yield and multiplying by 100%. Calculation of theoretical yield:
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Without proper ventilation and limited oxygen, the reaction of carbon and oxygen produces carbon monoxide.
2C(g) + O2(g) 2CO(g)
What is the percent yield if 40.0 g of CO is produced when 30.0 g of O2 is used?
Learning Check
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What is the percent yield if 40.0 g of CO is produced when 30.0 g of O2 is used?2C(g) + O2(g) 2CO(g)
30.0 g 40.0 g Actual yield ? Theoretical yield
Step 1 Write the given and needed quantities. Given: 30.0 g of O2, 40.0 g of CO Need: Theoretical yield, CO
Percent yield, CO
Solution
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2C(g) + O2(g) 2CO(g) 30.0 g 40.0 g Actual yield
? Theoretical yield
Step 2 Write a plan to calculate the theoretical and percent yield.
Solution
grams of O2
Molar MassMolar Mass
moles of O2
Molar MassMolar Mass
moles of CO
grams of CO
Mole–Mole factor
Mole–Mole factor
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2C(g) + O2(g) 2CO(g) 30.0 g 40.0 g Actual yield
? Theoretical yield
Step 3 Write the molar mass and mole–mole factors. 1 mole of O2 = 32.00 g of O2
Solution
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2C(g) + O2(g) 2CO(g) 30.0 g 40.0 g Actual yield
? Theoretical yield
Step 3 Write the molar mass and mole–mole factors.
1 mole of CO = 28.01 g of CO
Solution
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2C(g) + O2(g) 2CO(g) 30.0 g 40.0 g Actual yield
? Theoretical yield
Step 3 Write the molar mass and mole–mole factors. 1 mole of O2 = 2 moles of CO
Solution
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© 2014 Pearson Education, Inc.
2C(g) + O2(g) 2CO(g) 30.0 g 40.0 g Actual yield
? Theoretical yield
Step 4 Calculate the percent yield by dividing the actual yield by the theoretical yield and multiplying by 100%. Calculation of theoretical yield:
Solution
![Page 18: Chapter 9 Lecture Basic Chemistry Fourth Edition 9.4 Percent Yield Learning Goal Given the actual quantity of product, determine the percent yield for](https://reader035.vdocument.in/reader035/viewer/2022062217/5697c0251a28abf838cd553f/html5/thumbnails/18.jpg)
© 2014 Pearson Education, Inc.
2C(g) + O2(g) 2CO(g) 30.0 g 40.0 g Actual yield
? Theoretical yield
Step 4 Calculate the percent yield by dividing the actual yield by the theoretical yield and multiplying by 100%. Calculation of theoretical yield:
Solution