Solutions containing 5.07 g of aluminum chloride and 2.71 g of silver nitrate are combined to form 1.00 g of solid product. What is the percent yield in this reaction? Note: to receive full credit, your work must also show the limiting reactant and theoretical yield for the reaction, clearly labeled
Solutions containing 5.07 g of aluminum chloride and 2.71 g of silver nitrate are combined to form 1.00 g of solid product. What is the percent yield in this reaction? Note: to receive full credit, your work must also show the limiting reactant and theoretical yield for the reaction, clearly labeled
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
![---
**Determining the Percent Yield of a Chemical Reaction**
**Problem Statement:**
Solutions containing 5.07 g of aluminum chloride and 2.71 g of silver nitrate are combined to form 1.00 g of solid product. What is the percent yield in this reaction?
**Note:** To receive full credit, your work must also show the limiting reactant and theoretical yield for the reaction, clearly labeled.
---
### Explanation
To solve this problem, take the following steps:
1. **Identify the Reactants and Products:**
- Aluminum chloride (AlCl₃)
- Silver nitrate (AgNO₃)
- Solid product (assume it is either AgCl or another solid formed in this reaction)
2. **Determine the Balanced Chemical Equation:**
- Write the balanced chemical reaction that might occur when aluminum chloride reacts with silver nitrate.
3. **Calculate Moles of Each Reactant:**
- Calculate the number of moles for each reactant using the given masses and their molar masses.
4. **Identify the Limiting Reactant:**
- Determine which reactant is the limiting reagent by using stoichiometry.
5. **Calculate the Theoretical Yield:**
- Use the limiting reactant to calculate the theoretical yield of the product.
6. **Calculate the Percent Yield:**
- Use the following formula to determine the percent yield:
\[
\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\%
\]
### Steps in Detail:
1. **Balanced Chemical Equation:**
AlCl₃ + 3AgNO₃ → 3AgCl + Al(NO₃)₃
2. **Moles Calculation:**
- Molar mass of AlCl₃ = 133.34 g/mol
- Moles of AlCl₃ = 5.07 g / 133.34 g/mol
- Molar mass of AgNO₃ = 169.87 g/mol
- Moles of AgNO₃ = 2.71 g / 169.87 g/mol
3. **Limiting Reactant:**
- Use the stoichiometric coefficients from the balanced equation to identify the limiting reactant.
4. **Theoretical Yield:**
- Find the theoretical yield of](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1877c09b-7e56-4ac7-b3db-5c177db21a6d%2Fc016036e-c469-4c8d-b0ed-696b13ad1ffd%2Fus9t2hj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:---
**Determining the Percent Yield of a Chemical Reaction**
**Problem Statement:**
Solutions containing 5.07 g of aluminum chloride and 2.71 g of silver nitrate are combined to form 1.00 g of solid product. What is the percent yield in this reaction?
**Note:** To receive full credit, your work must also show the limiting reactant and theoretical yield for the reaction, clearly labeled.
---
### Explanation
To solve this problem, take the following steps:
1. **Identify the Reactants and Products:**
- Aluminum chloride (AlCl₃)
- Silver nitrate (AgNO₃)
- Solid product (assume it is either AgCl or another solid formed in this reaction)
2. **Determine the Balanced Chemical Equation:**
- Write the balanced chemical reaction that might occur when aluminum chloride reacts with silver nitrate.
3. **Calculate Moles of Each Reactant:**
- Calculate the number of moles for each reactant using the given masses and their molar masses.
4. **Identify the Limiting Reactant:**
- Determine which reactant is the limiting reagent by using stoichiometry.
5. **Calculate the Theoretical Yield:**
- Use the limiting reactant to calculate the theoretical yield of the product.
6. **Calculate the Percent Yield:**
- Use the following formula to determine the percent yield:
\[
\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\%
\]
### Steps in Detail:
1. **Balanced Chemical Equation:**
AlCl₃ + 3AgNO₃ → 3AgCl + Al(NO₃)₃
2. **Moles Calculation:**
- Molar mass of AlCl₃ = 133.34 g/mol
- Moles of AlCl₃ = 5.07 g / 133.34 g/mol
- Molar mass of AgNO₃ = 169.87 g/mol
- Moles of AgNO₃ = 2.71 g / 169.87 g/mol
3. **Limiting Reactant:**
- Use the stoichiometric coefficients from the balanced equation to identify the limiting reactant.
4. **Theoretical Yield:**
- Find the theoretical yield of
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