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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![### Chemical Reaction Calculation
**Question:**
How many grams of iron oxide are produced from 15.0 L of oxygen at STP? (Fe₂O₃ = 159.7 g/mol)
**Given Reaction:**
\[2 \text{Fe}_2\text{O}_3 \rightarrow 4 \text{Fe} + 3 \text{O}_2\]
### Explanation:
1. **Understanding STP:**
- STP stands for Standard Temperature and Pressure, which is 0°C (273.15 K) and 1 atm pressure.
- At STP, 1 mole of any gas occupies 22.4 liters.
2. **Finding Moles of O₂:**
- Volume of oxygen given = 15.0 L
- Using the molar volume at STP:
\[
\text{Moles of O}_2 = \frac{\text{Volume}}{\text{Molar Volume}} = \frac{15.0 \, \text{L}}{22.4 \, \text{L/mol}} = 0.669 \, \text{mol}
\]
3. **Using the Stoichiometric Coefficients:**
- According to the reaction:
- 3 moles of O₂ produce 2 moles of Fe₂O₃.
- Therefore, the moles of Fe₂O₃ produced can be calculated by:
\[
\text{Moles of Fe}_2\text{O}_3 = \frac{2}{3} \times \text{Moles of O}_2 = \frac{2}{3} \times 0.669 \, \text{mol} = 0.446 \, \text{mol}
\]
4. **Calculating the Mass of Fe₂O₃:**
- Molecular weight of Fe₂O₃ = 159.7 g/mol
Mass of Fe₂O₃ can be found as:
\[
\text{Mass of Fe}_2\text{O}_3 = \text{Moles} \times \text{Molar Mass} = 0.446 \, \text{mol} \times 159.7 \, \text{g/mol} = 71.25 \, \text{g}
\]
###](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb223a19b-0fd0-443c-881a-6f762159fad5%2F08d9d87e-2bd1-4560-8f10-1ddc6a936a9a%2Fw55im5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction Calculation
**Question:**
How many grams of iron oxide are produced from 15.0 L of oxygen at STP? (Fe₂O₃ = 159.7 g/mol)
**Given Reaction:**
\[2 \text{Fe}_2\text{O}_3 \rightarrow 4 \text{Fe} + 3 \text{O}_2\]
### Explanation:
1. **Understanding STP:**
- STP stands for Standard Temperature and Pressure, which is 0°C (273.15 K) and 1 atm pressure.
- At STP, 1 mole of any gas occupies 22.4 liters.
2. **Finding Moles of O₂:**
- Volume of oxygen given = 15.0 L
- Using the molar volume at STP:
\[
\text{Moles of O}_2 = \frac{\text{Volume}}{\text{Molar Volume}} = \frac{15.0 \, \text{L}}{22.4 \, \text{L/mol}} = 0.669 \, \text{mol}
\]
3. **Using the Stoichiometric Coefficients:**
- According to the reaction:
- 3 moles of O₂ produce 2 moles of Fe₂O₃.
- Therefore, the moles of Fe₂O₃ produced can be calculated by:
\[
\text{Moles of Fe}_2\text{O}_3 = \frac{2}{3} \times \text{Moles of O}_2 = \frac{2}{3} \times 0.669 \, \text{mol} = 0.446 \, \text{mol}
\]
4. **Calculating the Mass of Fe₂O₃:**
- Molecular weight of Fe₂O₃ = 159.7 g/mol
Mass of Fe₂O₃ can be found as:
\[
\text{Mass of Fe}_2\text{O}_3 = \text{Moles} \times \text{Molar Mass} = 0.446 \, \text{mol} \times 159.7 \, \text{g/mol} = 71.25 \, \text{g}
\]
###
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