1. A technician carries out several trials of a reaction that produces solid antimony, Sb(s). a) What is the percentage yield in each case? Trial 1: theoretical yield = 3.33 g Sb; actual yield = 3.02 g Sb percentage yield = Trial 2: theoretical yield = 5.82 g Sb; actual yield = 4.01 g Sb percentage yield = _% Trial 3: theoretical yield = 2.05 g Sb; actual yield = 1.95 g Sb percentage yield = b) Which trial would you consider the most efficient? Explain your answer.
1. A technician carries out several trials of a reaction that produces solid antimony, Sb(s). a) What is the percentage yield in each case? Trial 1: theoretical yield = 3.33 g Sb; actual yield = 3.02 g Sb percentage yield = Trial 2: theoretical yield = 5.82 g Sb; actual yield = 4.01 g Sb percentage yield = _% Trial 3: theoretical yield = 2.05 g Sb; actual yield = 1.95 g Sb percentage yield = b) Which trial would you consider the most efficient? Explain your answer.
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![1. A technician carries out several trials of a reaction that produces solid antimony, Sb(s).
a) What is the percentage yield in each case?
Trial 1: theoretical yield = 3.33 g Sb; actual yield = 3.02 g Sb
percentage yield =
Trial 2: theoretical yield = 5.82 g Sb; actual yield = 4.01 g Sb
percentage yield =
_%
Trial 3: theoretical yield = 2.05 g Sb; actual yield = 1.95 g Sb
percentage yield =
b) Which trial would you consider the most efficient? Explain your answer.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc5e173a7-a1ba-4f87-838e-f2e2de4f6c30%2F8689f04b-087a-42a0-ab29-b51ac40b9c18%2Fwygwuj_processed.png&w=3840&q=75)
Transcribed Image Text:1. A technician carries out several trials of a reaction that produces solid antimony, Sb(s).
a) What is the percentage yield in each case?
Trial 1: theoretical yield = 3.33 g Sb; actual yield = 3.02 g Sb
percentage yield =
Trial 2: theoretical yield = 5.82 g Sb; actual yield = 4.01 g Sb
percentage yield =
_%
Trial 3: theoretical yield = 2.05 g Sb; actual yield = 1.95 g Sb
percentage yield =
b) Which trial would you consider the most efficient? Explain your answer.
![2. For a demonstration, a teacher dissolves 5.38 g of potassium iodide, KI, in water, and adds an excess of
lead(II) nitrate, Pb(NO,), dissolved in water, to the solution. The reaction proceeds as shown in the
chemical equation below.
Pb(NO,),(aq) + 2KI(aq) → 2KNO,(aq) + Pbl.(s)
After filtering and drying the precipitate, the teacher determines that 7.02 g of lead(II) iodide, Pbls, have
been produced.
a) What is the theoretical yield of Pbl:(s)?
b) What is the percentage yield of Pbl:(s)?
Copyright © 2014 McGraw-Hil Ryerson
978-1-25-927538-8
Chemistry 12 College Preparation Worksheet
DATE
CLASS
CHAPTER 6
WKS Topic 6.7-2
Percentage Yield
Practice Problems
WORKSHEET
3. A student heats 2.05 g of calcium carbonate, CaCO.(s) so that it decomposes according to the chemical
equation below. After the reaction, the student measures 1.38 g of solid product.
CaCO.(s) → CaO(s) + CO:(g)
a) What is the theoretical yield of solid product?
b) What is the percentage yield of solid product?
c) What is one possible explanation for the answer to part b)?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc5e173a7-a1ba-4f87-838e-f2e2de4f6c30%2F8689f04b-087a-42a0-ab29-b51ac40b9c18%2Fau7pq0f_processed.png&w=3840&q=75)
Transcribed Image Text:2. For a demonstration, a teacher dissolves 5.38 g of potassium iodide, KI, in water, and adds an excess of
lead(II) nitrate, Pb(NO,), dissolved in water, to the solution. The reaction proceeds as shown in the
chemical equation below.
Pb(NO,),(aq) + 2KI(aq) → 2KNO,(aq) + Pbl.(s)
After filtering and drying the precipitate, the teacher determines that 7.02 g of lead(II) iodide, Pbls, have
been produced.
a) What is the theoretical yield of Pbl:(s)?
b) What is the percentage yield of Pbl:(s)?
Copyright © 2014 McGraw-Hil Ryerson
978-1-25-927538-8
Chemistry 12 College Preparation Worksheet
DATE
CLASS
CHAPTER 6
WKS Topic 6.7-2
Percentage Yield
Practice Problems
WORKSHEET
3. A student heats 2.05 g of calcium carbonate, CaCO.(s) so that it decomposes according to the chemical
equation below. After the reaction, the student measures 1.38 g of solid product.
CaCO.(s) → CaO(s) + CO:(g)
a) What is the theoretical yield of solid product?
b) What is the percentage yield of solid product?
c) What is one possible explanation for the answer to part b)?
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