Combining 0.205 mol Fe₂O3 with excess carbon produced 19.4 g Fe. Fe₂O3 + 3C 2 Fe + 3 CO What is the actual yield of iron in moles? actual yield: What is the theoretical yield of iron in moles? theoretical yield: What is the percent yield? percent yield: mol mol %
Combining 0.205 mol Fe₂O3 with excess carbon produced 19.4 g Fe. Fe₂O3 + 3C 2 Fe + 3 CO What is the actual yield of iron in moles? actual yield: What is the theoretical yield of iron in moles? theoretical yield: What is the percent yield? percent yield: mol mol %
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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Question
![**Chemical Reaction Yield Calculation**
**Scenario:**
Combining 0.205 mol of \( \text{Fe}_2\text{O}_3 \) with excess carbon produced 19.4 g of Fe.
**Reaction Equation:**
\[ \text{Fe}_2\text{O}_3 + 3 \text{C} \rightarrow 2 \text{Fe} + 3 \text{CO} \]
**Questions:**
1. **What is the actual yield of iron in moles?**
- **Actual yield:** [Enter value] mol
2. **What is the theoretical yield of iron in moles?**
- **Theoretical yield:** [Enter value] mol
3. **What is the percent yield?**
- **Percent yield:** [Enter value] %
**Instructions:**
- Calculate the moles of iron obtained using the actual weight given.
- Determine the maximum amount of iron that could be produced based on stoichiometry (theoretical yield).
- Calculate the percent yield using the formula:
\[
\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\%
\]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdc07c092-5f49-4d93-b501-b08294061775%2F1311a575-a88f-4aa1-ba56-ebac4ab20143%2Fpc4zgel_processed.png&w=3840&q=75)
Transcribed Image Text:**Chemical Reaction Yield Calculation**
**Scenario:**
Combining 0.205 mol of \( \text{Fe}_2\text{O}_3 \) with excess carbon produced 19.4 g of Fe.
**Reaction Equation:**
\[ \text{Fe}_2\text{O}_3 + 3 \text{C} \rightarrow 2 \text{Fe} + 3 \text{CO} \]
**Questions:**
1. **What is the actual yield of iron in moles?**
- **Actual yield:** [Enter value] mol
2. **What is the theoretical yield of iron in moles?**
- **Theoretical yield:** [Enter value] mol
3. **What is the percent yield?**
- **Percent yield:** [Enter value] %
**Instructions:**
- Calculate the moles of iron obtained using the actual weight given.
- Determine the maximum amount of iron that could be produced based on stoichiometry (theoretical yield).
- Calculate the percent yield using the formula:
\[
\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\%
\]
Expert Solution
Step 1
Fe2O3 + 3C → 2 Fe + 3 CO
0.205 mol Fe2O3 combines with excess carbon and produced 19.4 g Fe
We have to calculate the actual yield of iron , Theoretical yield of iron and percent of yield.
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