5. A student reacts 6.00 g of ammonium sulfide with 6.00 g of zinc (II) acetate. Upon completion of the experiment, their product weighs 2.41 g. What is the theoretical yield, actual yield and percent yield?
5. A student reacts 6.00 g of ammonium sulfide with 6.00 g of zinc (II) acetate. Upon completion of the experiment, their product weighs 2.41 g. What is the theoretical yield, actual yield and 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...
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![**Chemistry Problem: Yield Calculation**
*Problem Statement:*
A student reacts 6.00 g of ammonium sulfide with 6.00 g of zinc (II) acetate. Upon completion of the experiment, their product weighs 2.41 g. What is the theoretical yield, actual yield, and percent yield?
*Explanation:*
In this problem, the student is conducting a chemical reaction between ammonium sulfide (NH₄)₂S and zinc (II) acetate Zn(CH₃COO)₂. To solve for the theoretical yield, actual yield, and percent yield, the following steps should be taken:
1. **Determine the Limiting Reagent:**
- Calculate the moles of each reactant based on their given masses and molar masses.
2. **Calculate Theoretical Yield:**
- Use stoichiometry to determine the amount of product that can be formed from the limiting reagent.
3. **Identify Actual Yield:**
- The actual yield is given in the problem statement as 2.41 g.
4. **Calculate Percent Yield:**
- Use the formula:
\[
\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100
\]
By following these steps, students can fully understand the process of calculating yield in a chemical reaction.
*Note:* Detailed calculations involving molar masses, stoichiometric ratios, and conversion factors would typically follow in a classroom or homework setting to find the precise theoretical and percent yields.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7b0fedb7-adbc-492c-aa14-9f5d12342848%2F0b9ec3e3-f226-4c42-829d-a36eadddf399%2Ff97ps3o_processed.png&w=3840&q=75)
Transcribed Image Text:**Chemistry Problem: Yield Calculation**
*Problem Statement:*
A student reacts 6.00 g of ammonium sulfide with 6.00 g of zinc (II) acetate. Upon completion of the experiment, their product weighs 2.41 g. What is the theoretical yield, actual yield, and percent yield?
*Explanation:*
In this problem, the student is conducting a chemical reaction between ammonium sulfide (NH₄)₂S and zinc (II) acetate Zn(CH₃COO)₂. To solve for the theoretical yield, actual yield, and percent yield, the following steps should be taken:
1. **Determine the Limiting Reagent:**
- Calculate the moles of each reactant based on their given masses and molar masses.
2. **Calculate Theoretical Yield:**
- Use stoichiometry to determine the amount of product that can be formed from the limiting reagent.
3. **Identify Actual Yield:**
- The actual yield is given in the problem statement as 2.41 g.
4. **Calculate Percent Yield:**
- Use the formula:
\[
\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100
\]
By following these steps, students can fully understand the process of calculating yield in a chemical reaction.
*Note:* Detailed calculations involving molar masses, stoichiometric ratios, and conversion factors would typically follow in a classroom or homework setting to find the precise theoretical and percent yields.
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