Balancing Chemical Equation | PDF | Hydroxide | Sodium Hydroxide - Free Printable

Let's solve the Balancing Chemical Equations Worksheet step by step and then classify each reaction type.

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🔧 Step 1: Balancing Each Equation

We'll balance each chemical equation by ensuring the number of atoms of each element is equal on both sides.

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#### 1. Zn (s) + AgNO₃ (aq) → Zn(NO₃)₂ (aq) + Ag (s)

- Zn: 1 on left, 1 on right ✔
- Ag: 1 on left, 1 on right → but Ag is produced as solid, and Zn(NO₃)₂ has two NO₃⁻ groups.
- So need 2 AgNO₃ to provide two NO₃⁻ for Zn²⁺.

✔ Balanced:
Zn (s) + 2AgNO₃ (aq) → Zn(NO₃)₂ (aq) + 2Ag (s)

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#### 2. N₂ (g) + H₂ (g) → NH₃ (g)

- N₂ → 2N, NH₃ has 1N → need 2NH₃
- Then H: 2H₂ = 4H → 2NH₃ has 6H → need 3H₂

✔ Balanced:
N₂ (g) + 3H₂ (g) → 2NH₃ (g)

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#### 3. NaCl (aq) + AgC₂H₃O₂ (aq) → NaC₂H₃O₂ (aq) + AgCl (s)

- All ions exchange: double displacement
- One-to-one ratio: Na⁺, Cl⁻, Ag⁺, C₂H₃O₂⁻

✔ Balanced:
NaCl (aq) + AgC₂H₃O₂ (aq) → NaC₂H₃O₂ (aq) + AgCl (s)

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#### 4. Mg(OH)₂ (aq) + H₃PO₄ (aq) → H₂O (l) + Mg₃(PO₄)₂ (aq)

- Mg: 2 on left → 3 on right → LCM = 6
- So: 3Mg(OH)₂ and 2Mg₃(PO₄)₂ → wait, no: Mg₃(PO₄)₂ has 3 Mg → so need 3 Mg(OH)₂
- PO₄: H₃PO₄ → one per molecule; Mg₃(PO₄)₂ needs 2 PO₄ → so 2 H₃PO₄
- Now: 3Mg(OH)₂ + 2H₃PO₄ → Mg₃(PO₄)₂ + H₂O
- H: Left: 3×2 = 6H from OH, plus 2×3 = 6H from H₃PO₄ → total 12H
- Right: H₂O → need 6H₂O

✔ Balanced:
3Mg(OH)₂ (aq) + 2H₃PO₄ (aq) → 6H₂O (l) + Mg₃(PO₄)₂ (aq)

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#### 5. HNO₃ (aq) + Ni (s) → Ni(NO₃)₂ (aq) + H₂ (g)

- Ni: 1 → 1 ✔
- NO₃⁻: 2 in product → so need 2HNO₃
- H: 2H → H₂ gas → 2H → H₂

✔ Balanced:
2HNO₃ (aq) + Ni (s) → Ni(NO₃)₂ (aq) + H₂ (g)

> Note: This is a redox reaction where Ni displaces H⁺.

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#### 6. Ba(HCO₃)₂ (s) → BaCO₃ (s) + H₂O (g) + CO₂ (g)

- Decomposition of bicarbonate
- Ba(HCO₃)₂ → BaCO₃ + H₂O + CO₂
- But HCO₃⁻ decomposes: 2HCO₃⁻ → CO₃²⁻ + H₂O + CO₂
- So: Ba(HCO₃)₂ → BaCO₃ + H₂O + CO₂

✔ Already balanced:
Ba(HCO₃)₂ (s) → BaCO₃ (s) + H₂O (g) + CO₂ (g)

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#### 7. BaCl₂ (aq) + Na₂SO₄ (aq) → NaCl (aq) + BaSO₄ (s)

- Ba: 1 → 1 ✔
- SO₄: 1 → 1 ✔
- Na: 2 on left → need 2NaCl
- Cl: 2 on left → 2NaCl has 2Cl ✔

✔ Balanced:
BaCl₂ (aq) + Na₂SO₄ (aq) → 2NaCl (aq) + BaSO₄ (s)

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#### 8. Al₂(CO₃)₃ (s) → Al₂O₃ (s) + CO₂ (g)

- Decomposition
- CO₃²⁻ → CO₂ + O²⁻
- Al₂(CO₃)₃ has 3 CO₃ → 3CO₂
- O: Al₂O₃ has 3O, CO₂ has 6O → total 9O
- Left: Al₂(CO₃)₃ → 3×3 = 9O ✔

✔ Balanced:
Al₂(CO₃)₃ (s) → Al₂O₃ (s) + 3CO₂ (g)

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#### 9. Ca (s) + H₂O (l) → Ca(OH)₂ (aq) + H₂ (g)

- Ca: 1 → 1 ✔
- H: 2H₂O → 2H on left, but Ca(OH)₂ has 2H, H₂ has 2H → total 4H → need 2H₂O
- O: 2O → Ca(OH)₂ has 2O ✔

✔ Balanced:
Ca (s) + 2H₂O (l) → Ca(OH)₂ (aq) + H₂ (g)

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#### 10. LiHCO₃ (s) → Li₂CO₃ (s) + H₂O (g) + CO₂ (g)

- Li: 1 on left → 2 on right → need 2LiHCO₃
- HCO₃⁻: 2 → 2HCO₃⁻ → decompose to: CO₃²⁻ + H₂O + CO₂
- So: 2LiHCO₃ → Li₂CO₃ + H₂O + CO₂

✔ Balanced:
2LiHCO₃ (s) → Li₂CO₃ (s) + H₂O (g) + CO₂ (g)

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#### 11. N₂ (g) + O₂ (g) → N₂O₅ (g)

- N₂: 2N → N₂O₅ has 2N → good
- O₂: 5O needed → need 5/2 O₂ → multiply all by 2

✔ Balanced:
2N₂ (g) + 5O₂ (g) → 2N₂O₅ (g)

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#### 12. MgBr₂ (aq) + KOH (aq) → KBr (aq) + Mg(OH)₂ (s)

- Mg: 1 → 1 ✔
- Br: 2 → need 2KBr
- K: 2 → need 2KOH
- OH: 2 → Mg(OH)₂ needs 2OH → 2KOH provides 2OH ✔

✔ Balanced:
MgBr₂ (aq) + 2KOH (aq) → 2KBr (aq) + Mg(OH)₂ (s)

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#### 13. Mn (s) + CuCl₂ (aq) → Cu (s) + MnCl₂ (s)

- Mn: 1 → 1 ✔
- Cu: 1 → 1 ✔
- Cl: 2 → 2 ✔

✔ Balanced:
Mn (s) + CuCl₂ (aq) → Cu (s) + MnCl₂ (s)

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#### 14. Zn (s) + S₈ (s) → ZnS (s)

- S₈ has 8 S atoms → need 8ZnS
- So 8Zn needed

✔ Balanced:
8Zn (s) + S₈ (s) → 8ZnS (s)

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#### 15. NaOH (aq) + H₂SO₄ (aq) → H₂O (l) + Na₂SO₄ (aq)

- Na: 1 on left → 2 on right → need 2NaOH
- H: 2NaOH has 2H, H₂SO₄ has 2H → total 4H → 2H₂O
- SO₄: 1 → 1 ✔

✔ Balanced:
2NaOH (aq) + H₂SO₄ (aq) → 2H₂O (l) + Na₂SO₄ (aq)

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#### 16. K (s) + H₂O (l) → KOH (aq) + H₂ (g)

- K: 1 → 1 ✔
- H: 2H₂O → 2H, but KOH has 1H, H₂ has 2H → total 3H → not balanced
- Try 2K: 2K + 2H₂O → 2KOH + H₂
- H: 4H → 2KOH has 2H, H₂ has 2H → 4H ✔
- O: 2 → 2 ✔

✔ Balanced:
2K (s) + 2H₂O (l) → 2KOH (aq) + H₂ (g)

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#### 17. C₆H₁₂ (l) + O₂ (g) → H₂O (g) + CO₂ (g)

- Combustion: hydrocarbon + O₂ → CO₂ + H₂O
- C₆H₁₂ → 6C → 6CO₂
- H₁₂ → 6H₂O
- O: 6CO₂ has 12O, 6H₂O has 6O → total 18O → need 9O₂

✔ Balanced:
C₆H₁₂ (l) + 9O₂ (g) → 6H₂O (g) + 6CO₂ (g)

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#### 18. KOH (aq) + H₂CO₃ (aq) → H₂O (l) + K₂CO₃ (aq)

- K: 1 → 2 → need 2KOH
- H: 2KOH has 2H, H₂CO₃ has 2H → total 4H → 2H₂O
- CO₃: 1 → 1 ✔

✔ Balanced:
2KOH (aq) + H₂CO₃ (aq) → 2H₂O (l) + K₂CO₃ (aq)

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#### 19. C₆H₁₂O₆ (l) + O₂ (g) → H₂O (g) + CO₂ (g)

- Glucose combustion
- C₆H₁₂O₆ → 6C → 6CO₂
- H₁₂ → 6H₂O
- O: Left: 6 (from glucose) + 2x (from O₂)
- Right: 6CO₂ → 12O, 6H₂O → 6O → total 18O
- So: 6 + 2x = 18 → x = 6

✔ Balanced:
C₆H₁₂O₆ (l) + 6O₂ (g) → 6H₂O (g) + 6CO₂ (g)

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#### 20. Al (s) + S₈ (s) → Al₂S₃ (s)

- Al: 2 → need 2Al
- S: S₈ has 8S → Al₂S₃ has 3S → LCM of 8 and 3 = 24
- So: 4Al₂S₃ → 8Al, 12S → need 3/4 S₈? No
- Better: 8Al₂S₃ → 16Al, 24S → need 3S₈ (24S), and 16Al

So:
16Al + 3S₈ → 8Al₂S₃

✔ Balanced:
16Al (s) + 3S₈ (s) → 8Al₂S₃ (s)

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## ✔ Final Balanced Equations:

| # | Balanced Equation |
|---|-------------------|
| 1 | Zn + 2AgNO₃ → Zn(NO₃)₂ + 2Ag |
| 2 | N₂ + 3H₂ → 2NH₃ |
| 3 | NaCl + AgC₂H₃O₂ → NaC₂H₃O₂ + AgCl |
| 4 | 3Mg(OH)₂ + 2H₃PO₄ → 6H₂O + Mg₃(PO₄)₂ |
| 5 | 2HNO₃ + Ni → Ni(NO₃)₂ + H₂ |
| 6 | Ba(HCO₃)₂ → BaCO₃ + H₂O + CO₂ |
| 7 | BaCl₂ + Na₂SO₄ → 2NaCl + BaSO₄ |
| 8 | Al₂(CO₃)₃ → Al₂O₃ + 3CO₂ |
| 9 | Ca + 2H₂O → Ca(OH)₂ + H₂ |
|10 | 2LiHCO₃ → Li₂CO₃ + H₂O + CO₂ |
|11 | 2N₂ + 5O₂ → 2N₂O₅ |
|12 | MgBr₂ + 2KOH → 2KBr + Mg(OH)₂ |
|13 | Mn + CuCl₂ → Cu + MnCl₂ |
|14 | 8Zn + S₈ → 8ZnS |
|15 | 2NaOH + H₂SO₄ → 2H₂O + Na₂SO₄ |
|16 | 2K + 2H₂O → 2KOH + H₂ |
|17 | C₆H₁₂ + 9O₂ → 6H₂O + 6CO₂ |
|18 | 2KOH + H₂CO₃ → 2H₂O + K₂CO₃ |
|19 | C₆H₁₂O₆ + 6O₂ → 6H₂O + 6CO₂ |
|20 | 16Al + 3S₈ → 8Al₂S₃ |

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## 🧪 TYPES OF REACTION

The 5 main types of chemical reactions are:

1. Synthesis (Combination): A + B → AB
Example: 2H₂ + O₂ → 2H₂O

2. Decomposition: AB → A + B
Example: 2H₂O → 2H₂ + O₂

3. Single Replacement (Displacement): A + BC → AC + B
Example: Zn + 2HCl → ZnCl₂ + H₂

4. Double Replacement (Metathesis): AB + CD → AD + CB
Example: AgNO₃ + NaCl → AgCl + NaNO₃

5. Combustion: Hydrocarbon + O₂ → CO₂ + H₂O
Example: CH₄ + 2O₂ → CO₂ + 2H₂O

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## 🔍 Classify Each Reaction:

Now, classify the 20 reactions:

| # | Type |
|---|------|
| 1 | Single Replacement (Zn replaces Ag) |
| 2 | Synthesis (N₂ + H₂ → NH₃) |
| 3 | Double Replacement (ions swap) |
| 4 | Double Replacement (acid-base neutralization) |
| 5 | Single Replacement (Ni replaces H⁺) |
| 6 | Decomposition (bicarbonate breaks down) |
| 7 | Double Replacement (precipitation) |
| 8 | Decomposition (carbonate breaks down) |
| 9 | Single Replacement (Ca replaces H⁺) |
|10 | Decomposition (bicarbonate → carbonate + CO₂ + H₂O) |
|11 | Synthesis (N₂ + O₂ → N₂O₅) |
|12 | Double Replacement (precipitation of Mg(OH)₂) |
|13 | Single Replacement (Mn replaces Cu) |
|14 | Synthesis (Zn + S → ZnS) |
|15 | Double Replacement (acid-base) |
|16 | Single Replacement (K replaces H⁺) |
|17 | Combustion (hydrocarbon + O₂) |
|18 | Double Replacement (acid-base) |
|19 | Combustion (glucose + O₂) |
|20 | Synthesis (Al + S → Al₂S₃) |

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## ✔ Final Answer Summary:

Balanced Equations (Already shown above)

Types of Reactions (Listed above)

Classification of Reactions:

| # | Type |
|---|------|
| 1 | Single Replacement |
| 2 | Synthesis |
| 3 | Double Replacement |
| 4 | Double Replacement |
| 5 | Single Replacement |
| 6 | Decomposition |
| 7 | Double Replacement |
| 8 | Decomposition |
| 9 | Single Replacement |
|10 | Decomposition |
|11 | Synthesis |
|12 | Double Replacement |
|13 | Single Replacement |
|14 | Synthesis |
|15 | Double Replacement |
|16 | Single Replacement |
|17 | Combustion |
|18 | Double Replacement |
|19 | Combustion |
|20 | Synthesis |

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