A student named Jack precipitated lead ions from solution using the following reaction Pb (aq) + 2 NaCl(aq) PbCl2(s) + 2 Na*(aq) He added excess NaCi (aq) to a solution containing 195.7 g of Pbions. The precipitate that formed was found to have a mass of 252.4 g. Other students, reporting a 100% yield, obtained 262.7 g of PbCl2 product. What was Jack's percent yield?
A student named Jack precipitated lead ions from solution using the following reaction Pb (aq) + 2 NaCl(aq) PbCl2(s) + 2 Na*(aq) He added excess NaCi (aq) to a solution containing 195.7 g of Pbions. The precipitate that formed was found to have a mass of 252.4 g. Other students, reporting a 100% yield, obtained 262.7 g of PbCl2 product. What was Jack's percent yield?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Question
100%
What was Jack's percentage yield?
![## Percent Yield Calculation in Precipitation Reaction
A student named Jack precipitated lead ions from a solution using the following reaction:
\[ \text{Pb}^{2+}(aq) + 2 \text{NaCl}(aq) \rightarrow \text{PbCl}_2(s) + 2 \text{Na}^+(aq) \]
He added excess \(\text{NaCl}(aq)\) to a solution containing \(195.7 \, \text{g}\) of \(\text{Pb}^{2+}\) ions. The precipitate that formed was found to have a mass of \(252.4 \, \text{g}\). Other students, reporting a \(100\%\) yield, obtained \(262.7 \, \text{g}\) of \(\text{PbCl}_2\) product. What was Jack's percent yield?
#### Options:
- O 104.1%
- O 74.50%
- O 77.54%
- O 96.08% (Selected)
### Solution Explanation:
Calculating the percent yield of a chemical reaction involves comparing the actual yield to the theoretical yield using the formula:
\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\% \]
Given data:
- Theoretical Yield = \(262.7 \, \text{g}\)
- Actual Yield (Jack's) = \(252.4 \, \text{g}\)
Calculation:
\[ \text{Percent Yield} = \left( \frac{252.4 \, \text{g}}{262.7 \, \text{g}} \right) \times 100\% \approx 96.08\% \]
Hence, Jack's percent yield is accurately calculated as 96.08%.
For additional visual representation:
- No graphs or diagrams are included in the provided text.
This example teaches students how to calculate the percent yield of a reaction, which is an essential concept in stoichiometry and experimental chemistry.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7a2b26e2-0834-47d0-a095-02bbc56be37a%2F14cfd7c2-b4c2-4f5d-ada3-408a2665d12c%2Ftvgw6aa.jpeg&w=3840&q=75)
Transcribed Image Text:## Percent Yield Calculation in Precipitation Reaction
A student named Jack precipitated lead ions from a solution using the following reaction:
\[ \text{Pb}^{2+}(aq) + 2 \text{NaCl}(aq) \rightarrow \text{PbCl}_2(s) + 2 \text{Na}^+(aq) \]
He added excess \(\text{NaCl}(aq)\) to a solution containing \(195.7 \, \text{g}\) of \(\text{Pb}^{2+}\) ions. The precipitate that formed was found to have a mass of \(252.4 \, \text{g}\). Other students, reporting a \(100\%\) yield, obtained \(262.7 \, \text{g}\) of \(\text{PbCl}_2\) product. What was Jack's percent yield?
#### Options:
- O 104.1%
- O 74.50%
- O 77.54%
- O 96.08% (Selected)
### Solution Explanation:
Calculating the percent yield of a chemical reaction involves comparing the actual yield to the theoretical yield using the formula:
\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\% \]
Given data:
- Theoretical Yield = \(262.7 \, \text{g}\)
- Actual Yield (Jack's) = \(252.4 \, \text{g}\)
Calculation:
\[ \text{Percent Yield} = \left( \frac{252.4 \, \text{g}}{262.7 \, \text{g}} \right) \times 100\% \approx 96.08\% \]
Hence, Jack's percent yield is accurately calculated as 96.08%.
For additional visual representation:
- No graphs or diagrams are included in the provided text.
This example teaches students how to calculate the percent yield of a reaction, which is an essential concept in stoichiometry and experimental chemistry.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY