An organic chemistry student performed a synthesis of benzoic acid using a Grignard reagent. The following experimental data were collected: 0.5438 g 0.6000 g 0.3842 g Bromobenzene used Magnesium Benzoic acid obtained Write all of the reactions leading to the final isolated product. Calculate the % yield of benzoic acid.
An organic chemistry student performed a synthesis of benzoic acid using a Grignard reagent. The following experimental data were collected: 0.5438 g 0.6000 g 0.3842 g Bromobenzene used Magnesium Benzoic acid obtained Write all of the reactions leading to the final isolated product. Calculate the % yield of benzoic acid.
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%
stuck in organic chem
![**Title: Synthesis of Benzoic Acid Using a Grignard Reagent**
An organic chemistry student performed a synthesis of benzoic acid using a Grignard reagent. The following experimental data were collected:
- Bromobenzene used: 0.5438 g
- Magnesium: 0.6000 g
- Benzoic acid obtained: 0.3842 g
**Instructions:**
1. **Write all of the reactions leading to the final isolated product.**
(Note: This section requires the student to delineate the step-by-step chemical reactions that transform bromobenzene into the final product of benzoic acid via a Grignard reagent.)
2. **Calculate the % yield of benzoic acid.**
(Note: The percentage yield is calculated by comparing the actual yield (amount of product obtained from the experiment) to the theoretical yield (the amount of product expected according to stoichiometric calculations).)
Formula for Percent Yield Calculation:
\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \]
**Steps and Considerations:**
- Establish the balanced chemical equations for each stage of the synthesis process.
- Determine the molar masses of the reactants and products.
- Calculate the moles of reactants used and the theoretical yield of the product based on stoichiometry.
- Use the provided experimental yield (0.3842 g) to find the percent yield by applying the formula above.
---
**Calculated Percentage Yield Example:**
Given:
- Actual yield of benzoic acid (obtained): 0.3842 g
- Using experimental data and balanced reactions, the theoretical yield needs to be calculated first.
**Detailed Example Calculation:**
1. Write and balance the chemical equation.
2. Convert grams of bromobenzene used to moles (Molar mass of bromobenzene ≈ 157.01 g/mol).
3. Convert grams of magnesium used to moles (Molar mass of magnesium ≈ 24.305 g/mol).
4. Using stoichiometry, calculate the theoretical moles of benzoic acid producible.
5. Convert the theoretical moles of benzoic acid to grams (Molar mass of benzoic acid ≈ 122.12 g/mol).
6. Calculate the percent yield using the mentioned formula.
**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F206206aa-1104-4dbc-9e08-21639f631eee%2Faefd5da4-3d03-489c-b6da-0e2c3c82b92b%2F05jz7nc_processed.png&w=3840&q=75)
Transcribed Image Text:**Title: Synthesis of Benzoic Acid Using a Grignard Reagent**
An organic chemistry student performed a synthesis of benzoic acid using a Grignard reagent. The following experimental data were collected:
- Bromobenzene used: 0.5438 g
- Magnesium: 0.6000 g
- Benzoic acid obtained: 0.3842 g
**Instructions:**
1. **Write all of the reactions leading to the final isolated product.**
(Note: This section requires the student to delineate the step-by-step chemical reactions that transform bromobenzene into the final product of benzoic acid via a Grignard reagent.)
2. **Calculate the % yield of benzoic acid.**
(Note: The percentage yield is calculated by comparing the actual yield (amount of product obtained from the experiment) to the theoretical yield (the amount of product expected according to stoichiometric calculations).)
Formula for Percent Yield Calculation:
\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \]
**Steps and Considerations:**
- Establish the balanced chemical equations for each stage of the synthesis process.
- Determine the molar masses of the reactants and products.
- Calculate the moles of reactants used and the theoretical yield of the product based on stoichiometry.
- Use the provided experimental yield (0.3842 g) to find the percent yield by applying the formula above.
---
**Calculated Percentage Yield Example:**
Given:
- Actual yield of benzoic acid (obtained): 0.3842 g
- Using experimental data and balanced reactions, the theoretical yield needs to be calculated first.
**Detailed Example Calculation:**
1. Write and balance the chemical equation.
2. Convert grams of bromobenzene used to moles (Molar mass of bromobenzene ≈ 157.01 g/mol).
3. Convert grams of magnesium used to moles (Molar mass of magnesium ≈ 24.305 g/mol).
4. Using stoichiometry, calculate the theoretical moles of benzoic acid producible.
5. Convert the theoretical moles of benzoic acid to grams (Molar mass of benzoic acid ≈ 122.12 g/mol).
6. Calculate the percent yield using the mentioned formula.
**
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 with 2 images
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