If 0.315 g of AI (26.982 g/mol) is reacted in the synthesis of Alum reaction and 3.265 g of Alum (474.39 g/mol) is produced, determine the percent yield. O 60% O 58% O 57% O 55% O 59% O 56%
If 0.315 g of AI (26.982 g/mol) is reacted in the synthesis of Alum reaction and 3.265 g of Alum (474.39 g/mol) is produced, determine the percent yield. O 60% O 58% O 57% O 55% O 59% O 56%
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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![**Problem Statement:**
If 0.315 g of Al (26.982 g/mol) is reacted in the synthesis of Alum reaction and 3.265 g of Alum (474.39 g/mol) is produced, determine the percent yield.
**Options:**
- ○ 60%
- ○ 58%
- ○ 57%
- ○ 55%
- ○ 59%
- ○ 56%
**Solution Explanation:**
To determine the percent yield, follow these steps:
1. **Calculate moles of Aluminum (Al):**
\[
\text{Moles of Al} = \frac{0.315 \, \text{g}}{26.982 \, \text{g/mol}}
\]
2. **Calculate theoretical yield of Alum:**
Determine the moles of Alum that should theoretically form from the moles of Al using the stoichiometry of the reaction, if provided.
3. **Calculate actual moles of Alum produced:**
\[
\text{Moles of Alum} = \frac{3.265 \, \text{g}}{474.39 \, \text{g/mol}}
\]
4. **Calculate percent yield:**
\[
\text{Percent Yield} = \left( \frac{\text{Actual Moles}}{\text{Theoretical Moles}} \right) \times 100
\]
Use these steps to find the correct percent yield from the given options.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff405cacd-b73c-4ff5-aae6-a678a4b84912%2F9da7403f-1598-4e50-98bf-9041d6908641%2Fb4zhhvu_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
If 0.315 g of Al (26.982 g/mol) is reacted in the synthesis of Alum reaction and 3.265 g of Alum (474.39 g/mol) is produced, determine the percent yield.
**Options:**
- ○ 60%
- ○ 58%
- ○ 57%
- ○ 55%
- ○ 59%
- ○ 56%
**Solution Explanation:**
To determine the percent yield, follow these steps:
1. **Calculate moles of Aluminum (Al):**
\[
\text{Moles of Al} = \frac{0.315 \, \text{g}}{26.982 \, \text{g/mol}}
\]
2. **Calculate theoretical yield of Alum:**
Determine the moles of Alum that should theoretically form from the moles of Al using the stoichiometry of the reaction, if provided.
3. **Calculate actual moles of Alum produced:**
\[
\text{Moles of Alum} = \frac{3.265 \, \text{g}}{474.39 \, \text{g/mol}}
\]
4. **Calculate percent yield:**
\[
\text{Percent Yield} = \left( \frac{\text{Actual Moles}}{\text{Theoretical Moles}} \right) \times 100
\]
Use these steps to find the correct percent yield from the given options.
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