2) If iron(II) sulfate is heated too strongly, the following reaction will occur FeSO4(s) FeO(s) + SO3(g) If you are heating a sample of FeSO4 6H2O and this reaction occurs along with dehydration, what will happen to the experimental percent water? Explain your answer. visynon tro
2) If iron(II) sulfate is heated too strongly, the following reaction will occur FeSO4(s) FeO(s) + SO3(g) If you are heating a sample of FeSO4 6H2O and this reaction occurs along with dehydration, what will happen to the experimental percent water? Explain your answer. visynon tro
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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![**Text Transcription for Educational Website**
### Reactions and Calculations with Hydrates
**1. Aluminum Chloride Hexahydrate**
\[ \text{Aluminum Chloride Hexahydrate: } \text{AlCl}_3 \cdot 6\text{H}_2\text{O} \]
- **AlCl₃ Molecular Weight:** 133.34 g/mol
- **AlCl₃·6H₂O Molecular Weight Calculation:**
\[ 133.34 + 6(18.02) = 241.46 \, \text{g/mol} \]
- **Percentage of Water (Th\%):**
\[
\text{Th\%} = \left( \frac{6(18.02)}{241.46} \right) \times 100\% = 44.78\%
\]
**2. Reaction of Iron(II) Sulfate**
- **Reaction:**
\[ \text{FeSO}_4(s) \rightarrow \text{FeO}(s) + \text{SO}_3(g) \]
- If you heat a sample of FeSO₄·6H₂O and this reaction occurs along with dehydration, the experimental percent water will likely decrease since SO₃ is released as a gas, indicating additional weight loss beyond water alone.
**3. Determining Water Content in Calcium Chloride Hydrate**
- **Given:** 8.416 g sample of CaCl₂·xH₂O; 5.624 g remains after heating.
- **Mass of H₂O lost:**
\[ 8.416 \, \text{g} - 5.624 \, \text{g} = 2.792 \, \text{g} \]
- **Moles of H₂O:**
\[ 2.792 \, \text{g} \times \left( \frac{1 \, \text{mol}}{18.02 \, \text{g}} \right) = 0.1549 \, \text{mol} \]
- **Moles of CaCl₂:**
\[ 5.624 \, \text{g} \times \left( \frac{1 \, \text{mol}}{110.98 \, \text{](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe7a54da2-bb36-4266-99d7-672b4d4e9da7%2Fd9bc456e-a2e6-41c8-94f8-fd321e86c2ea%2F683ap6k_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Text Transcription for Educational Website**
### Reactions and Calculations with Hydrates
**1. Aluminum Chloride Hexahydrate**
\[ \text{Aluminum Chloride Hexahydrate: } \text{AlCl}_3 \cdot 6\text{H}_2\text{O} \]
- **AlCl₃ Molecular Weight:** 133.34 g/mol
- **AlCl₃·6H₂O Molecular Weight Calculation:**
\[ 133.34 + 6(18.02) = 241.46 \, \text{g/mol} \]
- **Percentage of Water (Th\%):**
\[
\text{Th\%} = \left( \frac{6(18.02)}{241.46} \right) \times 100\% = 44.78\%
\]
**2. Reaction of Iron(II) Sulfate**
- **Reaction:**
\[ \text{FeSO}_4(s) \rightarrow \text{FeO}(s) + \text{SO}_3(g) \]
- If you heat a sample of FeSO₄·6H₂O and this reaction occurs along with dehydration, the experimental percent water will likely decrease since SO₃ is released as a gas, indicating additional weight loss beyond water alone.
**3. Determining Water Content in Calcium Chloride Hydrate**
- **Given:** 8.416 g sample of CaCl₂·xH₂O; 5.624 g remains after heating.
- **Mass of H₂O lost:**
\[ 8.416 \, \text{g} - 5.624 \, \text{g} = 2.792 \, \text{g} \]
- **Moles of H₂O:**
\[ 2.792 \, \text{g} \times \left( \frac{1 \, \text{mol}}{18.02 \, \text{g}} \right) = 0.1549 \, \text{mol} \]
- **Moles of CaCl₂:**
\[ 5.624 \, \text{g} \times \left( \frac{1 \, \text{mol}}{110.98 \, \text{
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