What is the maximum number of grams of Ag that can be produced if 0.570 mol of Zn and 0.691 mo of Ag,0 react? Zn(s) + Ag,0(s) → ZnO(s) + 2 Ag(s) 1 2 Based on your knowledge of stoichiometry, set up the table below to determine the amounts of each reactant and product after the reaction goes to completion. Zn(s) + Ag20(s) → ZnO(s) + 2 Ag(s) Before (mol) Change (mol)
What is the maximum number of grams of Ag that can be produced if 0.570 mol of Zn and 0.691 mo of Ag,0 react? Zn(s) + Ag,0(s) → ZnO(s) + 2 Ag(s) 1 2 Based on your knowledge of stoichiometry, set up the table below to determine the amounts of each reactant and product after the reaction goes to completion. Zn(s) + Ag20(s) → ZnO(s) + 2 Ag(s) Before (mol) Change (mol)
Chemistry
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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
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![**Stoichiometry Problem: Reaction of Zn and Ag₂O**
**Question:**
Consider the balanced chemical reaction below. What is the maximum number of grams of Ag that can be produced if 0.570 mol of Zn and 0.691 mol of Ag₂O react?
\[ \text{Zn(s)} + \text{Ag}_2\text{O(s)} \rightarrow \text{ZnO(s)} + 2 \text{Ag(s)} \]
**Solution:**
Given the balanced equation, analyze the stoichiometry to determine the amounts of each reactant and product after the reaction goes to completion.
**Stoichiometric Coefficients:**
- \( \text{Zn(s)} \) : 1
- \( \text{Ag}_2\text{O(s)} \) : 1
- \( \text{ZnO(s)} \) : 1
- \( \text{Ag(s)} \) : 2
**Reaction Table:**
| | Zn(s) | + | Ag₂O(s) | → | ZnO(s) | + | 2 Ag(s) |
|---------|-------|---|---------|---|--------|---|---------|
| **Before (mol)** | | | | | | | |
| **Change (mol)** | | | | | | | |
| **After (mol)** | | | | | | | |
**Solution Options:**
- Option 1:
- Before: 0.570 mol (Zn), 0.691 mol (Ag₂O)
- Change: -0.570 mol (Zn), -0.285 mol (Ag₂O)
- After: 0 mol (Zn), 0.406 mol (Ag₂O), 0.570 mol (ZnO), 1.140 mol (Ag)
- Option 2:
- Before: 0.570 mol (Zn), 0.691 mol (Ag₂O)
- Change: -0.285 mol (Zn), -0.691 mol (Ag₂O)
- After: 0.285 mol (Zn), 0 mol (Ag₂O), 0.285 mol (ZnO), 1.382 mol (Ag)
**Conclusion:**
Determine the](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1e4f7fd3-dbae-49c8-b999-a719c9747eb1%2Fe5dd6f25-9304-469c-baf8-83465ea97a4a%2Fcel3nrh_processed.png&w=3840&q=75)
Transcribed Image Text:**Stoichiometry Problem: Reaction of Zn and Ag₂O**
**Question:**
Consider the balanced chemical reaction below. What is the maximum number of grams of Ag that can be produced if 0.570 mol of Zn and 0.691 mol of Ag₂O react?
\[ \text{Zn(s)} + \text{Ag}_2\text{O(s)} \rightarrow \text{ZnO(s)} + 2 \text{Ag(s)} \]
**Solution:**
Given the balanced equation, analyze the stoichiometry to determine the amounts of each reactant and product after the reaction goes to completion.
**Stoichiometric Coefficients:**
- \( \text{Zn(s)} \) : 1
- \( \text{Ag}_2\text{O(s)} \) : 1
- \( \text{ZnO(s)} \) : 1
- \( \text{Ag(s)} \) : 2
**Reaction Table:**
| | Zn(s) | + | Ag₂O(s) | → | ZnO(s) | + | 2 Ag(s) |
|---------|-------|---|---------|---|--------|---|---------|
| **Before (mol)** | | | | | | | |
| **Change (mol)** | | | | | | | |
| **After (mol)** | | | | | | | |
**Solution Options:**
- Option 1:
- Before: 0.570 mol (Zn), 0.691 mol (Ag₂O)
- Change: -0.570 mol (Zn), -0.285 mol (Ag₂O)
- After: 0 mol (Zn), 0.406 mol (Ag₂O), 0.570 mol (ZnO), 1.140 mol (Ag)
- Option 2:
- Before: 0.570 mol (Zn), 0.691 mol (Ag₂O)
- Change: -0.285 mol (Zn), -0.691 mol (Ag₂O)
- After: 0.285 mol (Zn), 0 mol (Ag₂O), 0.285 mol (ZnO), 1.382 mol (Ag)
**Conclusion:**
Determine the
![**Stoichiometry Practice: Determining Maximum Amount of Iron Production**
**Question 17 of 20**
Consider the balanced chemical reaction below. What is the maximum amount of grams of Fe that can be produced from 33.4 g of iron(III) oxide mixed with 47.2 g of carbon monoxide?
\[ \text{Fe}_2\text{O}_3(s) + 3 \text{CO}(g) \rightarrow 2 \text{Fe}(s) + 3 \text{CO}_2(g) \]
Use the table below to determine the amounts of each reactant and product after the reaction goes to completion.
| | Fe<sub>2</sub>O<sub>3</sub>(s) | + | 3 CO(g) | → | 2 Fe(s) | + | 3 CO<sub>2</sub>(g) |
|-------|------------|---|-------|---|-----|---|--------|
| Before (mol) | 0.209 | | 1.69 | | 0 | | 0 |
| Change (mol) | -0.209 | | -1.69 | | 1.19 | | 0.627 |
| After (mol) | | | | | | | |
**Calculation Table**
- **Reactants and Products:**
- Iron(III) oxide (Fe<sub>2</sub>O<sub>3</sub>)
- Carbon monoxide (CO)
- Iron (Fe)
- Carbon dioxide (CO<sub>2</sub>)
- **Amount in Grams and Moles:**
- Starting values:
- Fe<sub>2</sub>O<sub>3</sub>: 33.4 g
- CO: 47.2 g
- Moles:
- Initial moles of Fe<sub>2</sub>O<sub>3</sub>: 0.209 mol
- Initial moles of CO: 1.69 mol
- Changes after reaction:
- Fe<sub>2</sub>O<sub>3</sub> is fully consumed: -0.209 mol
- CO is fully consumed: -1.69 mol
- Fe](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1e4f7fd3-dbae-49c8-b999-a719c9747eb1%2Fe5dd6f25-9304-469c-baf8-83465ea97a4a%2F7j7skv9_processed.png&w=3840&q=75)
Transcribed Image Text:**Stoichiometry Practice: Determining Maximum Amount of Iron Production**
**Question 17 of 20**
Consider the balanced chemical reaction below. What is the maximum amount of grams of Fe that can be produced from 33.4 g of iron(III) oxide mixed with 47.2 g of carbon monoxide?
\[ \text{Fe}_2\text{O}_3(s) + 3 \text{CO}(g) \rightarrow 2 \text{Fe}(s) + 3 \text{CO}_2(g) \]
Use the table below to determine the amounts of each reactant and product after the reaction goes to completion.
| | Fe<sub>2</sub>O<sub>3</sub>(s) | + | 3 CO(g) | → | 2 Fe(s) | + | 3 CO<sub>2</sub>(g) |
|-------|------------|---|-------|---|-----|---|--------|
| Before (mol) | 0.209 | | 1.69 | | 0 | | 0 |
| Change (mol) | -0.209 | | -1.69 | | 1.19 | | 0.627 |
| After (mol) | | | | | | | |
**Calculation Table**
- **Reactants and Products:**
- Iron(III) oxide (Fe<sub>2</sub>O<sub>3</sub>)
- Carbon monoxide (CO)
- Iron (Fe)
- Carbon dioxide (CO<sub>2</sub>)
- **Amount in Grams and Moles:**
- Starting values:
- Fe<sub>2</sub>O<sub>3</sub>: 33.4 g
- CO: 47.2 g
- Moles:
- Initial moles of Fe<sub>2</sub>O<sub>3</sub>: 0.209 mol
- Initial moles of CO: 1.69 mol
- Changes after reaction:
- Fe<sub>2</sub>O<sub>3</sub> is fully consumed: -0.209 mol
- CO is fully consumed: -1.69 mol
- Fe
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