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
Please help with question 6
![### Educational Exercise: Calculating Chemical Yields
#### Instructions:
1. **Calculate Mass of Sodium Carbonate:**
- To prepare a Sodium Carbonate (Na₂CO₃) solution from 100 mL of a 0.750 M solution, determine the mass required.
- **Solution:**
\[
\frac{100 \text{ mL}}{1000 \text{ mL/L}} \times 0.750 \text{ mol/L} = 0.075 \text{ mol}
\]
\[
\text{Na}_2\text{CO}_3 = 106 \text{ g/mol}
\]
\[
\text{Mass of Na}_2\text{CO}_3 = 106 \text{ g/mol} \times 0.075 \text{ mol} = 7.95 \text{ g}
\]
2. **Calculate Mass of Calcium Chloride:**
- To prepare a 0.250 M solution of CaCl₂ from 100 mL of solution, determine the mass of Calcium Chloride required.
- **Solution:**
\[
0.250 \text{ m} \times \frac{100 \text{ mL}}{1000 \text{ mL/L}} = 0.025 \text{ mol}
\]
3. **Calculate Theoretical Yield of Calcium Carbonate:**
- If using 10.0 mL of Sodium Carbonate solution with an excess of Calcium Chloride, determine how many grams of Calcium Carbonate should be theoretically produced.
- **Reaction:**
\[
\text{Na}_2\text{CO}_3 + \text{CaCl}_2 \rightarrow \text{CaCO}_3 + 2\text{NaCl}
\]
4. **Calculate Yield from Calcium Chloride Solution:**
- Using 25.0 mL of Calcium Chloride solution and an excess of Sodium Carbonate, calculate the theoretical yield of Calcium Carbonate.
5. **Determine Combined Theoretical Yield:**
- Using results from steps 3 and 4, find the theoretical yield when 25.0 mL of a 0.250 M solution of CaCl₂ is mixed with 10.0 mL of a 0.750 M Sodium Carbonate solution.
6](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6c605e87-2c96-4aa2-99a1-2c5d12ea3556%2F44621d2b-7666-4d4a-bf10-4a7d51a276b6%2Fzto72hp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Educational Exercise: Calculating Chemical Yields
#### Instructions:
1. **Calculate Mass of Sodium Carbonate:**
- To prepare a Sodium Carbonate (Na₂CO₃) solution from 100 mL of a 0.750 M solution, determine the mass required.
- **Solution:**
\[
\frac{100 \text{ mL}}{1000 \text{ mL/L}} \times 0.750 \text{ mol/L} = 0.075 \text{ mol}
\]
\[
\text{Na}_2\text{CO}_3 = 106 \text{ g/mol}
\]
\[
\text{Mass of Na}_2\text{CO}_3 = 106 \text{ g/mol} \times 0.075 \text{ mol} = 7.95 \text{ g}
\]
2. **Calculate Mass of Calcium Chloride:**
- To prepare a 0.250 M solution of CaCl₂ from 100 mL of solution, determine the mass of Calcium Chloride required.
- **Solution:**
\[
0.250 \text{ m} \times \frac{100 \text{ mL}}{1000 \text{ mL/L}} = 0.025 \text{ mol}
\]
3. **Calculate Theoretical Yield of Calcium Carbonate:**
- If using 10.0 mL of Sodium Carbonate solution with an excess of Calcium Chloride, determine how many grams of Calcium Carbonate should be theoretically produced.
- **Reaction:**
\[
\text{Na}_2\text{CO}_3 + \text{CaCl}_2 \rightarrow \text{CaCO}_3 + 2\text{NaCl}
\]
4. **Calculate Yield from Calcium Chloride Solution:**
- Using 25.0 mL of Calcium Chloride solution and an excess of Sodium Carbonate, calculate the theoretical yield of Calcium Carbonate.
5. **Determine Combined Theoretical Yield:**
- Using results from steps 3 and 4, find the theoretical yield when 25.0 mL of a 0.250 M solution of CaCl₂ is mixed with 10.0 mL of a 0.750 M Sodium Carbonate solution.
6
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