Noting the moles of reactants calculated above, as well as the mole ratios of Cu to each reactant, determine the following. Show all work. A) Theoretical moles Cu from CuSO4 b) Theoretical moles Cu from Al
Noting the moles of reactants calculated above, as well as the mole ratios of Cu to each reactant, determine the following. Show all work. A) Theoretical moles Cu from CuSO4 b) Theoretical moles Cu from Al
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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a. Noting the moles of reactants calculated above, as well as the mole ratios of Cu to each reactant, determine the following. Show all work.
A) Theoretical moles Cu from CuSO4
b) Theoretical moles Cu from Al
Transcribed Image Text:**Theoretical and Actual Yield of Copper (Cu)**
**1. Theoretical Yield of Cu in Moles**
- Calculated Yield: 0.078 moles
- Calculation: 0.052 moles * 3/2 = 0.078 moles
**2. Theoretical Yield of Cu in Grams**
- Calculated Yield: 4.95 grams
- Calculation: 0.078 mol * 63.5 g/mol = 4.95 grams
**3. Actual Yield of Cu in Grams**
- Measured Yield: 3.06 grams
- Calculation: 5.46 g - 2.40 g = 3.06 g
**4. Percent Yield of Cu**
- Calculated Yield: 162%
- Calculation: (4.95 g / 3.06 g) * 100 = 162%
This data outlines the theoretical and actual yields in a copper reaction. The percent yield calculation suggests the efficiency of the actual yield compared to the theoretical prediction.
![**Balanced Chemical Equation:**
\[ 2\text{Al}(s) + 3\text{CuSO}_4(aq) \rightarrow \text{Al}_2(\text{SO}_4)_3(aq) + 3\text{Cu}(s) \]
| **Parameter** | **Answer** | **Show Your Work** |
|-----------------------------------------------|-----------------|------------------------------------------------|
| **Volume of 1 M CuSO₄** | 100 ml | |
| **Mass of Al foil** | 1.4 g | |
| **Moles CuSO₄** | 0.0001 moles | \(= 1M \times 0.100 \, \text{L} = 0.0001 \, \text{moles}\) |
| **Moles of Al** | 0.052 moles | \(= \frac{1.4 \, \text{g}}{26.9815 \, \frac{\text{g}}{\text{mol}}} = 0.052 \, \text{moles}\) |
| **Moles Cu Product based on Starting CuSO₄** | 0.1 moles | CuSO₄ \(= 0.100 \, \text{mol} \times \frac{3}{3} = 0.1 \, \text{moles}\) |
| **Moles Cu Product based on Starting Al** | 0.078 moles | \(= 0.052 \, \text{moles} \times \frac{3}{2} = 0.078 \, \text{moles}\) |
| **Limiting Reactant** | Al (aluminum) | Al is the limiting reactant because 0.078 moles is less than 0.1 moles. Consuming Al first. |
This table guides you through the stoichiometric calculations for the reaction between aluminum and copper(II) sulfate. It identifies the limiting reactant as aluminum due to its lower mole amount, ensuring all aluminum is consumed first.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcb45a7b7-d1aa-4ac7-ad98-90aa0325071f%2F9643459f-3702-48d7-bd55-5bc38508f691%2Fje8leug_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Balanced Chemical Equation:**
\[ 2\text{Al}(s) + 3\text{CuSO}_4(aq) \rightarrow \text{Al}_2(\text{SO}_4)_3(aq) + 3\text{Cu}(s) \]
| **Parameter** | **Answer** | **Show Your Work** |
|-----------------------------------------------|-----------------|------------------------------------------------|
| **Volume of 1 M CuSO₄** | 100 ml | |
| **Mass of Al foil** | 1.4 g | |
| **Moles CuSO₄** | 0.0001 moles | \(= 1M \times 0.100 \, \text{L} = 0.0001 \, \text{moles}\) |
| **Moles of Al** | 0.052 moles | \(= \frac{1.4 \, \text{g}}{26.9815 \, \frac{\text{g}}{\text{mol}}} = 0.052 \, \text{moles}\) |
| **Moles Cu Product based on Starting CuSO₄** | 0.1 moles | CuSO₄ \(= 0.100 \, \text{mol} \times \frac{3}{3} = 0.1 \, \text{moles}\) |
| **Moles Cu Product based on Starting Al** | 0.078 moles | \(= 0.052 \, \text{moles} \times \frac{3}{2} = 0.078 \, \text{moles}\) |
| **Limiting Reactant** | Al (aluminum) | Al is the limiting reactant because 0.078 moles is less than 0.1 moles. Consuming Al first. |
This table guides you through the stoichiometric calculations for the reaction between aluminum and copper(II) sulfate. It identifies the limiting reactant as aluminum due to its lower mole amount, ensuring all aluminum is consumed first.
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