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Step-by-step solution for: Worksheet Predicting Products of Reactions Key | Exercises ...
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Step-by-step solution for: Worksheet Predicting Products of Reactions Key | Exercises ...
Here is the complete solution to the “Predicting Products of Chemical Reactions” worksheet, including predicted products, balanced equations, and reaction type identification where needed.
---
Combustion Reactions (a, b, c)
*All combustion reactions of organic compounds with O₂ produce CO₂ and H₂O.*
a. Combustion: C₆H₁₂ + O₂ →
→ C₆H₁₂ + 9O₂ → 6CO₂ + 6H₂O
*(Balanced: 6 C, 12 H, 18 O on each side)*
b. Combustion: C₄H₆ + O₂ →
→ 2C₄H₆ + 11O₂ → 8CO₂ + 6H₂O
*(Balanced: 8 C, 12 H, 22 O on each side)*
c. Combustion: C₆H₁₀O₃ + O₂ →
→ C₆H₁₀O₃ + 7O₂ → 6CO₂ + 5H₂O
*(Balanced: 6 C, 10 H, 17 O on each side — note: 3 from original compound + 14 from 7 O₂ = 17 O; products: 12 in 6CO₂ + 5 in 5H₂O = 17 O)*
---
1. Synthesis: Mg + I₂ →
Magnesium metal reacts with iodine to form magnesium iodide.
→ Mg + I₂ → MgI₂
*(Already balanced)*
---
2. Double displacement: CuCl₂ + H₂S →
Copper(II) chloride reacts with hydrogen sulfide to form copper(II) sulfide (insoluble precipitate) and HCl.
→ CuCl₂ + H₂S → CuS↓ + 2HCl
---
3. Double displacement: NaOH + HClO₄ →
Strong base + strong acid → salt + water (neutralization).
→ NaOH + HClO₄ → NaClO₄ + H₂O
*(Already balanced)*
---
4. Decomposition: ZnCO₃ + heat →
Metal carbonates decompose to metal oxide and CO₂.
→ ZnCO₃ → ZnO + CO₂
*(Already balanced)*
---
5. Single replacement: HCl + Zn →
Zinc displaces hydrogen from acid to form zinc chloride and H₂ gas.
→ 2HCl + Zn → ZnCl₂ + H₂
*(Balanced: 2 H, 2 Cl, 1 Zn on each side)*
---
6. Na + MgCl₂ →
This is a single replacement reaction. Sodium is more reactive than magnesium (check activity series), so it can displace Mg²⁺.
→ 2Na + MgCl₂ → 2NaCl + Mg
*(Balanced)*
---
7. CaCl₂ + K₂CO₃ →
Double displacement: forms CaCO₃ (insoluble) and KCl.
→ CaCl₂ + K₂CO₃ → CaCO₃↓ + 2KCl
*(Reaction type: Double displacement)*
---
8. K + Cl₂ →
Synthesis: potassium metal reacts with chlorine gas to form potassium chloride.
→ 2K + Cl₂ → 2KCl
*(Balanced; Reaction type: Synthesis)*
---
9. BaCl₂ + K₃PO₄ →
Double displacement: forms Ba₃(PO₄)₂ (insoluble) and KCl.
→ 3BaCl₂ + 2K₃PO₄ → Ba₃(PO₄)₂↓ + 6KCl
*(Reaction type: Double displacement)*
---
10. H₂SO₄ + KOH →
Acid-base neutralization → salt + water.
→ H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O
*(Reaction type: Double displacement / Neutralization)*
---
11. Al₂(CO₃)₃ + heat →
Decomposition of aluminum carbonate → aluminum oxide + CO₂.
→ Al₂(CO₃)₃ → Al₂O₃ + 3CO₂
*(Reaction type: Decomposition)*
---
12. Al + O₂ →
Synthesis: aluminum metal reacts with oxygen to form aluminum oxide.
→ 4Al + 3O₂ → 2Al₂O₃
*(Reaction type: Synthesis)*
---
13. Pb(NO₃)₂ + KOH →
Double displacement: forms Pb(OH)₂ (insoluble) and KNO₃.
→ Pb(NO₃)₂ + 2KOH → Pb(OH)₂↓ + 2KNO₃
*(Reaction type: Double displacement)*
---
14. H₂SO₄ + BaCl₂ →
Double displacement: forms BaSO₄ (insoluble) and HCl.
→ H₂SO₄ + BaCl₂ → BaSO₄↓ + 2HCl
*(Reaction type: Double displacement)*
---
15. Ca + AgCl →
Single replacement: calcium is more reactive than silver → displaces Ag⁺.
→ Ca + 2AgCl → CaCl₂ + 2Ag
*(Note: AgCl is solid, but reaction proceeds if Ca is molten or in contact; Reaction type: Single replacement)*
---
16. H₃PO₄ + FeBr₃ →
Double displacement: forms FePO₄ (insoluble) and HBr.
→ H₃PO₄ + FeBr₃ → FePO₄↓ + 3HBr
*(Reaction type: Double displacement)*
---
17. Li + N₂ →
Synthesis: lithium reacts with nitrogen to form lithium nitride.
→ 6Li + N₂ → 2Li₃N
*(Reaction type: Synthesis)*
---
18. HCl + Mg(OH)₂ →
Neutralization: acid + base → salt + water.
→ 2HCl + Mg(OH)₂ → MgCl₂ + 2H₂O
*(Reaction type: Double displacement / Neutralization)*
---
19. Mg(OH)₂ + heat →
Decomposition: metal hydroxides decompose to metal oxide + water.
→ Mg(OH)₂ → MgO + H₂O
*(Reaction type: Decomposition)*
---
20. Fe(OH)₃ + heat →
Decomposition: iron(III) hydroxide → iron(III) oxide + water.
→ 2Fe(OH)₃ → Fe₂O₃ + 3H₂O
*(Reaction type: Decomposition)*
---
✔ Summary of Reaction Types for Blank Lines (6–20):
| # | Reaction Type |
|---|------------------------|
| 6 | Single replacement |
| 7 | Double displacement |
| 8 | Synthesis |
| 9 | Double displacement |
|10 | Double displacement |
|11 | Decomposition |
|12 | Synthesis |
|13 | Double displacement |
|14 | Double displacement |
|15 | Single replacement |
|16 | Double displacement |
|17 | Synthesis |
|18 | Double displacement |
|19 | Decomposition |
|20 | Decomposition |
---
📌 Key Tips Used:
- Combustion: Always CO₂ + H₂O for hydrocarbons/oxygenated organics.
- Synthesis: Two elements → one compound.
- Decomposition: One compound → two or more products (often with heat).
- Single Replacement: A + BC → AC + B (use activity series).
- Double Displacement: AB + CD → AD + CB (look for precipitates, gases, or water).
Let me know if you’d like help balancing any equation step-by-step or understanding why a specific product forms!
---
Combustion Reactions (a, b, c)
*All combustion reactions of organic compounds with O₂ produce CO₂ and H₂O.*
a. Combustion: C₆H₁₂ + O₂ →
→ C₆H₁₂ + 9O₂ → 6CO₂ + 6H₂O
*(Balanced: 6 C, 12 H, 18 O on each side)*
b. Combustion: C₄H₆ + O₂ →
→ 2C₄H₆ + 11O₂ → 8CO₂ + 6H₂O
*(Balanced: 8 C, 12 H, 22 O on each side)*
c. Combustion: C₆H₁₀O₃ + O₂ →
→ C₆H₁₀O₃ + 7O₂ → 6CO₂ + 5H₂O
*(Balanced: 6 C, 10 H, 17 O on each side — note: 3 from original compound + 14 from 7 O₂ = 17 O; products: 12 in 6CO₂ + 5 in 5H₂O = 17 O)*
---
1. Synthesis: Mg + I₂ →
Magnesium metal reacts with iodine to form magnesium iodide.
→ Mg + I₂ → MgI₂
*(Already balanced)*
---
2. Double displacement: CuCl₂ + H₂S →
Copper(II) chloride reacts with hydrogen sulfide to form copper(II) sulfide (insoluble precipitate) and HCl.
→ CuCl₂ + H₂S → CuS↓ + 2HCl
---
3. Double displacement: NaOH + HClO₄ →
Strong base + strong acid → salt + water (neutralization).
→ NaOH + HClO₄ → NaClO₄ + H₂O
*(Already balanced)*
---
4. Decomposition: ZnCO₃ + heat →
Metal carbonates decompose to metal oxide and CO₂.
→ ZnCO₃ → ZnO + CO₂
*(Already balanced)*
---
5. Single replacement: HCl + Zn →
Zinc displaces hydrogen from acid to form zinc chloride and H₂ gas.
→ 2HCl + Zn → ZnCl₂ + H₂
*(Balanced: 2 H, 2 Cl, 1 Zn on each side)*
---
6. Na + MgCl₂ →
This is a single replacement reaction. Sodium is more reactive than magnesium (check activity series), so it can displace Mg²⁺.
→ 2Na + MgCl₂ → 2NaCl + Mg
*(Balanced)*
---
7. CaCl₂ + K₂CO₃ →
Double displacement: forms CaCO₃ (insoluble) and KCl.
→ CaCl₂ + K₂CO₃ → CaCO₃↓ + 2KCl
*(Reaction type: Double displacement)*
---
8. K + Cl₂ →
Synthesis: potassium metal reacts with chlorine gas to form potassium chloride.
→ 2K + Cl₂ → 2KCl
*(Balanced; Reaction type: Synthesis)*
---
9. BaCl₂ + K₃PO₄ →
Double displacement: forms Ba₃(PO₄)₂ (insoluble) and KCl.
→ 3BaCl₂ + 2K₃PO₄ → Ba₃(PO₄)₂↓ + 6KCl
*(Reaction type: Double displacement)*
---
10. H₂SO₄ + KOH →
Acid-base neutralization → salt + water.
→ H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O
*(Reaction type: Double displacement / Neutralization)*
---
11. Al₂(CO₃)₃ + heat →
Decomposition of aluminum carbonate → aluminum oxide + CO₂.
→ Al₂(CO₃)₃ → Al₂O₃ + 3CO₂
*(Reaction type: Decomposition)*
---
12. Al + O₂ →
Synthesis: aluminum metal reacts with oxygen to form aluminum oxide.
→ 4Al + 3O₂ → 2Al₂O₃
*(Reaction type: Synthesis)*
---
13. Pb(NO₃)₂ + KOH →
Double displacement: forms Pb(OH)₂ (insoluble) and KNO₃.
→ Pb(NO₃)₂ + 2KOH → Pb(OH)₂↓ + 2KNO₃
*(Reaction type: Double displacement)*
---
14. H₂SO₄ + BaCl₂ →
Double displacement: forms BaSO₄ (insoluble) and HCl.
→ H₂SO₄ + BaCl₂ → BaSO₄↓ + 2HCl
*(Reaction type: Double displacement)*
---
15. Ca + AgCl →
Single replacement: calcium is more reactive than silver → displaces Ag⁺.
→ Ca + 2AgCl → CaCl₂ + 2Ag
*(Note: AgCl is solid, but reaction proceeds if Ca is molten or in contact; Reaction type: Single replacement)*
---
16. H₃PO₄ + FeBr₃ →
Double displacement: forms FePO₄ (insoluble) and HBr.
→ H₃PO₄ + FeBr₃ → FePO₄↓ + 3HBr
*(Reaction type: Double displacement)*
---
17. Li + N₂ →
Synthesis: lithium reacts with nitrogen to form lithium nitride.
→ 6Li + N₂ → 2Li₃N
*(Reaction type: Synthesis)*
---
18. HCl + Mg(OH)₂ →
Neutralization: acid + base → salt + water.
→ 2HCl + Mg(OH)₂ → MgCl₂ + 2H₂O
*(Reaction type: Double displacement / Neutralization)*
---
19. Mg(OH)₂ + heat →
Decomposition: metal hydroxides decompose to metal oxide + water.
→ Mg(OH)₂ → MgO + H₂O
*(Reaction type: Decomposition)*
---
20. Fe(OH)₃ + heat →
Decomposition: iron(III) hydroxide → iron(III) oxide + water.
→ 2Fe(OH)₃ → Fe₂O₃ + 3H₂O
*(Reaction type: Decomposition)*
---
✔ Summary of Reaction Types for Blank Lines (6–20):
| # | Reaction Type |
|---|------------------------|
| 6 | Single replacement |
| 7 | Double displacement |
| 8 | Synthesis |
| 9 | Double displacement |
|10 | Double displacement |
|11 | Decomposition |
|12 | Synthesis |
|13 | Double displacement |
|14 | Double displacement |
|15 | Single replacement |
|16 | Double displacement |
|17 | Synthesis |
|18 | Double displacement |
|19 | Decomposition |
|20 | Decomposition |
---
📌 Key Tips Used:
- Combustion: Always CO₂ + H₂O for hydrocarbons/oxygenated organics.
- Synthesis: Two elements → one compound.
- Decomposition: One compound → two or more products (often with heat).
- Single Replacement: A + BC → AC + B (use activity series).
- Double Displacement: AB + CD → AD + CB (look for precipitates, gases, or water).
Let me know if you’d like help balancing any equation step-by-step or understanding why a specific product forms!
Parent Tip: Review the logic above to help your child master the concept of chemistry predicting products worksheet.
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