Worksheet for practicing balancing chemical equations and identifying reaction types.

Task Overview

The worksheet involves balancing chemical equations and identifying the types of reactions. Below, I will solve each equation step-by-step and then classify them into the five main types of chemical reactions.

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Balancing Chemical Equations

#### 1. Zn(s) + AgNO₃(aq) → Zn(NO₃)₂(aq) + Ag(s)
- Reactants: Zn, AgNO₃
- Products: Zn(NO₃)₂, Ag
- Balance:
- Start with zinc (Zn): 1 Zn on both sides.
- Balance silver (Ag): 1 Ag in AgNO₃ and 1 Ag in products → need 2 AgNO₃.
- Balance nitrate (NO₃⁻): 2 NO₃⁻ in products → need 2 AgNO₃.
- Final balanced equation:
Zn(s) + 2 AgNO₃(aq) → Zn(NO₃)₂(aq) + 2 Ag(s)

#### 2. N₂(g) + H₂(g) → NH₃(g)
- Reactants: N₂, H₂
- Products: NH₃
- Balance:
- Start with nitrogen (N): 2 N in N₂ and 1 N in NH₃ → need 2 NH₃.
- Balance hydrogen (H): 3 H in 2 NH₃ and 2 H in H₂ → need 3 H₂.
- Final balanced equation:
N₂(g) + 3 H₂(g) → 2 NH₃(g)

#### 3. NaCl(aq) + AgC₂H₃O₂(aq) → NaC₂H₃O₂(aq) + AgCl(s)
- Reactants: NaCl, AgC₂H₃O₂
- Products: NaC₂H₃O₂, AgCl
- Balance:
- All atoms are already balanced (1 Na, 1 Cl, 1 Ag, 1 C₂H₃O₂).
- Final balanced equation:
NaCl(aq) + AgC₂H₃O₂(aq) → NaC₂H₃O₂(aq) + AgCl(s)

#### 4. Mg(OH)₂(aq) + H₃PO₄(aq) → H₂O(l) + Mg₃(PO₄)₂(aq)
- Reactants: Mg(OH)₂, H₃PO₄
- Products: H₂O, Mg₃(PO₄)₂
- Balance:
- Balance magnesium (Mg): 3 Mg in Mg₃(PO₄)₂ → need 3 Mg(OH)₂.
- Balance phosphate (PO₄³⁻): 2 PO₄³⁻ in Mg₃(PO₄)₂ → need 2 H₃PO₄.
- Balance hydrogen (H): 6 H in 3 Mg(OH)₂ and 6 H in 2 H₃PO₄ → 6 H₂O.
- Final balanced equation:
3 Mg(OH)₂(aq) + 2 H₃PO₄(aq) → 6 H₂O(l) + Mg₃(PO₄)₂(aq)

#### 5. HNO₃(aq) + Ni(s) → Ni(NO₃)₂(aq) + H₂(g)
- Reactants: HNO₃, Ni
- Products: Ni(NO₃)₂, H₂
- Balance:
- Balance nickel (Ni): 1 Ni in Ni(NO₃)₂ → need 2 HNO₃.
- Balance nitrate (NO₃⁻): 2 NO₃⁻ in Ni(NO₃)₂ → need 2 HNO₃.
- Balance hydrogen (H): 2 H in 2 HNO₃ → 1 H₂.
- Final balanced equation:
2 HNO₃(aq) + Ni(s) → Ni(NO₃)₂(aq) + H₂(g)

#### 6. Ba(HCO₃)₂(s) → BaCO₃(s) + H₂O(g) + CO₂(g)
- Reactants: Ba(HCO₃)₂
- Products: BaCO₃, H₂O, CO₂
- Balance:
- All atoms are already balanced (1 Ba, 2 C, 6 O, 2 H).
- Final balanced equation:
Ba(HCO₃)₂(s) → BaCO₃(s) + H₂O(g) + CO₂(g)

#### 7. BaCl₂(aq) + Na₂SO₄(aq) → NaCl(aq) + BaSO₄(s)
- Reactants: BaCl₂, Na₂SO₄
- Products: NaCl, BaSO₄
- Balance:
- Balance barium (Ba): 1 Ba in BaCl₂ and 1 Ba in BaSO₄.
- Balance chlorine (Cl): 2 Cl in BaCl₂ → need 2 NaCl.
- Balance sodium (Na): 2 Na in Na₂SO₄ → need 2 NaCl.
- Final balanced equation:
BaCl₂(aq) + Na₂SO₄(aq) → 2 NaCl(aq) + BaSO₄(s)

#### 8. Al₂(CO₃)₃(s) → Al₂O₃(s) + CO₂(g)
- Reactants: Al₂(CO₃)₃
- Products: Al₂O₃, CO₂
- Balance:
- Balance aluminum (Al): 2 Al in Al₂(CO₃)₃ and Al₂O₃.
- Balance carbon (C): 3 C in Al₂(CO₃)₃ → need 3 CO₂.
- Balance oxygen (O): 9 O in Al₂(CO₃)₃ (3 CO₃²⁻) → 3 O in Al₂O₃ and 6 O in 3 CO₂.
- Final balanced equation:
Al₂(CO₃)₃(s) → Al₂O₃(s) + 3 CO₂(g)

#### 9. Ca(s) + H₂O(l) → Ca(OH)₂(aq) + H₂(g)
- Reactants: Ca, H₂O
- Products: Ca(OH)₂, H₂
- Balance:
- Balance calcium (Ca): 1 Ca in Ca(OH)₂ → need 1 Ca.
- Balance hydroxide (OH⁻): 2 OH⁻ in Ca(OH)₂ → need 2 H₂O.
- Balance hydrogen (H): 2 H in 2 H₂O → 1 H₂.
- Final balanced equation:
Ca(s) + 2 H₂O(l) → Ca(OH)₂(aq) + H₂(g)

#### 10. LiHCO₃(s) → Li₂CO₃(s) + H₂O(g) + CO₂(g)
- Reactants: LiHCO₃
- Products: Li₂CO₃, H₂O, CO₂
- Balance:
- Balance lithium (Li): 2 Li in Li₂CO₃ → need 2 LiHCO₃.
- Balance carbon (C): 1 C in LiHCO₃ → need 1 CO₂.
- Balance oxygen (O): 3 O in LiHCO₃ → 3 O in Li₂CO₃, 1 O in H₂O, and 2 O in CO₂.
- Final balanced equation:
2 LiHCO₃(s) → Li₂CO₃(s) + H₂O(g) + CO₂(g)

#### 11. N₂(g) + O₂(g) → N₂O₅(g)
- Reactants: N₂, O₂
- Products: N₂O₅
- Balance:
- Nitrogen (N): 2 N in N₂ and N₂O₅.
- Oxygen (O): 5 O in N₂O₅ → need 5/2 O₂ → multiply all coefficients by 2.
- Final balanced equation:
2 N₂(g) + 5 O₂(g) → 2 N₂O₅(g)

#### 12. MgBr₂(aq) + KOH(aq) → KBr(aq) + Mg(OH)₂(s)
- Reactants: MgBr₂, KOH
- Products: KBr, Mg(OH)₂
- Balance:
- Balance magnesium (Mg): 1 Mg in MgBr₂ and Mg(OH)₂.
- Balance bromide (Br⁻): 2 Br⁻ in MgBr₂ → need 2 KBr.
- Balance potassium (K): 2 K in 2 KBr → need 2 KOH.
- Balance hydroxide (OH⁻): 2 OH⁻ in 2 KOH → 2 OH⁻ in Mg(OH)₂.
- Final balanced equation:
MgBr₂(aq) + 2 KOH(aq) → 2 KBr(aq) + Mg(OH)₂(s)

#### 13. Mn(s) + CuCl₂(aq) → Cu(s) + MnCl₂(s)
- Reactants: Mn, CuCl₂
- Products: Cu, MnCl₂
- Balance:
- Balance manganese (Mn): 1 Mn in MnCl₂ → need 1 Mn.
- Balance copper (Cu): 1 Cu in CuCl₂ → need 1 Cu.
- Balance chloride (Cl⁻): 2 Cl⁻ in CuCl₂ → 2 Cl⁻ in MnCl₂.
- Final balanced equation:
Mn(s) + CuCl₂(aq) → Cu(s) + MnCl₂(s)

#### 14. Zn(s) + S₈(s) → ZnS(s)
- Reactants: Zn, S₈
- Products: ZnS
- Balance:
- Balance zinc (Zn): 1 Zn in ZnS → need 8 Zn.
- Balance sulfur (S): 8 S in S₈ → need 8 ZnS.
- Final balanced equation:
8 Zn(s) + S₈(s) → 8 ZnS(s)

#### 15. NaOH(aq) + H₂SO₄(aq) → H₂O(l) + Na₂SO₄(aq)
- Reactants: NaOH, H₂SO₄
- Products: H₂O, Na₂SO₄
- Balance:
- Balance sodium (Na): 2 Na in Na₂SO₄ → need 2 NaOH.
- Balance sulfate (SO₄²⁻): 1 SO₄²⁻ in H₂SO₄ and Na₂SO₄.
- Balance hydrogen (H): 2 H in H₂SO₄ → 2 H₂O.
- Balance oxygen (O): 4 O in H₂SO₄ and 4 O in 2 H₂O.
- Final balanced equation:
2 NaOH(aq) + H₂SO₄(aq) → 2 H₂O(l) + Na₂SO₄(aq)

#### 16. K(s) + H₂O(l) → KOH(aq) + H₂(g)
- Reactants: K, H₂O
- Products: KOH, H₂
- Balance:
- Balance potassium (K): 1 K in KOH → need 1 K.
- Balance hydroxide (OH⁻): 1 OH⁻ in KOH → need 1 H₂O.
- Balance hydrogen (H): 2 H in H₂O → 1 H₂.
- Final balanced equation:
2 K(s) + 2 H₂O(l) → 2 KOH(aq) + H₂(g)

#### 17. C₃H₁₂(l) + O₂(g) → H₂O(g) + CO₂(g)
- Reactants: C₃H₁₂, O₂
- Products: H₂O, CO₂
- Balance:
- Balance carbon (C): 3 C in C₃H₁₂ → need 3 CO₂.
- Balance hydrogen (H): 12 H in C₃H₁₂ → 6 H₂O.
- Balance oxygen (O): 3 O in 3 CO₂ + 6 O in 6 H₂O = 9 O → need 9/2 O₂ → multiply all coefficients by 2.
- Final balanced equation:
2 C₃H₁₂(l) + 21 O₂(g) → 12 H₂O(g) + 6 CO₂(g)

#### 18. KOH(aq) + H₂CO₃(aq) → H₂O(l) + K₂CO₃(aq)
- Reactants: KOH, H₂CO₃
- Products: H₂O, K₂CO₃
- Balance:
- Balance potassium (K): 2 K in K₂CO₃ → need 2 KOH.
- Balance carbonate (CO₃²⁻): 1 CO₃²⁻ in H₂CO₃ and K₂CO₃.
- Balance hydrogen (H): 2 H in H₂CO₃ → 2 H₂O.
- Final balanced equation:
2 KOH(aq) + H₂CO₃(aq) → 2 H₂O(l) + K₂CO₃(aq)

#### 19. C₄H₁₀(l) + O₂(g) → H₂O(g) + CO₂(g)
- Reactants: C₄H₁₀, O₂
- Products: H₂O, CO₂
- Balance:
- Balance carbon (C): 4 C in C₄H₁₀ → need 4 CO₂.
- Balance hydrogen (H): 10 H in C₄H₁₀ → 5 H₂O.
- Balance oxygen (O): 4 O in 4 CO₂ + 5 O in 5 H₂O = 9 O → need 9/2 O₂ → multiply all coefficients by 2.
- Final balanced equation:
2 C₄H₁₀(l) + 13 O₂(g) → 10 H₂O(g) + 8 CO₂(g)

#### 20. Al(s) + S₈(s) → Al₂S₃(s)
- Reactants: Al, S₈
- Products: Al₂S₃
- Balance:
- Balance aluminum (Al): 2 Al in Al₂S₃ → need 2 Al.
- Balance sulfur (S): 3 S in Al₂S₃ → need 3/8 S₈ → multiply all coefficients by 8.
- Final balanced equation:
16 Al(s) + 2 S₈(s) → 8 Al₂S₃(s)

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Types of Reactions

The five main types of chemical reactions are:
1. Synthesis Reaction: Two or more substances combine to form one product.
- Example: \( \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \)

2. Decomposition Reaction: One substance breaks down into two or more simpler substances.
- Example: \( \text{Ba(HCO}_3)_2(s) \rightarrow \text{BaCO}_3(s) + \text{H}_2\text{O}(g) + \text{CO}_2(g) \)

3. Single Displacement Reaction: One element replaces another in a compound.
- Example: \( \text{Zn}(s) + 2\text{AgNO}_3(aq) \rightarrow \text{Zn(NO}_3)_2(aq) + 2\text{Ag}(s) \)

4. Double Displacement Reaction: Ions from two compounds switch places to form two new compounds.
- Example: \( \text{BaCl}_2(aq) + \text{Na}_2\text{SO}_4(aq) \rightarrow 2\text{NaCl}(aq) + \text{BaSO}_4(s) \)

5. Combustion Reaction: A substance reacts with oxygen to produce heat and light.
- Example: \( \text{C}_4\text{H}_{10}(l) + \frac{13}{2}\text{O}_2(g) \rightarrow 5\text{H}_2\text{O}(g) + 4\text{CO}_2(g) \)

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Classification of Reactions

| Reaction Number | Type of Reaction | Balanced Equation |
|-----------------|--------------------------------------|-----------------------------------------------------------------------------------|
| 1 | Single Displacement | \( \text{Zn}(s) + 2\text{AgNO}_3(aq) \rightarrow \text{Zn(NO}_3)_2(aq) + 2\text{Ag}(s) \) |
| 2 | Synthesis | \( \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \) |
| 3 | Double Displacement | \( \text{NaCl}(aq) + \text{AgC}_2\text{H}_3\text{O}_2(aq) \rightarrow \text{NaC}_2\text{H}_3\text{O}_2(aq) + \text{AgCl}(s) \) |
| 4 | Double Displacement | \( 3\text{Mg(OH)}_2(aq) + 2\text{H}_3\text{PO}_4(aq) \rightarrow 6\text{H}_2\text{O}(l) + \text{Mg}_3(\text{PO}_4)_2(aq) \) |
| 5 | Single Displacement | \( 2\text{HNO}_3(aq) + \text{Ni}(s) \rightarrow \text{Ni(NO}_3)_2(aq) + \text{H}_2(g) \) |
| 6 | Decomposition | \( \text{Ba(HCO}_3)_2(s) \rightarrow \text{BaCO}_3(s) + \text{H}_2\text{O}(g) + \text{CO}_2(g) \) |
| 7 | Double Displacement | \( \text{BaCl}_2(aq) + \text{Na}_2\text{SO}_4(aq) \rightarrow 2\text{NaCl}(aq) + \text{BaSO}_4(s) \) |
| 8 | Decomposition | \( \text{Al}_2(\text{CO}_3)_3(s) \rightarrow \text{Al}_2\text{O}_3(s) + 3\text{CO}_2(g) \) |
| 9 | Single Displacement | \( \text{Ca}(s) + 2\text{H}_2\text{O}(l) \rightarrow \text{Ca(OH)}_2(aq) + \text{H}_2(g) \) |
| 10 | Decomposition | \( 2\text{LiHCO}_3(s) \rightarrow \text{Li}_2\text{CO}_3(s) + \text{H}_2\text{O}(g) + \text{CO}_2(g) \) |
| 11 | Synthesis | \( 2\text{N}_2(g) + 5\text{O}_2(g) \rightarrow 2\text{N}_2\text{O}_5(g) \) |
| 12 | Double Displacement | \( \text{MgBr}_2(aq) + 2\text{KOH}(aq) \rightarrow 2\text{KBr}(aq) + \text{Mg(OH)}_2(s) \) |
| 13 | Single Displacement | \( \text{Mn}(s) + \text{CuCl}_2(aq) \rightarrow \text{Cu}(s) + \text{MnCl}_2(s) \) |
| 14 | Synthesis | \( 8\text{Zn}(s) + \text{S}_8(s) \rightarrow 8\text{ZnS}(s) \) |
| 15 | Double Displacement | \( 2\text{NaOH}(aq) + \text{H}_2\text{SO}_4(aq) \rightarrow 2\text{H}_2\text{O}(l) + \text{Na}_2\text{SO}_4(aq) \) |
| 16 | Single Displacement | \( 2\text{K}(s) + 2\text{H}_2\text{O}(l) \rightarrow 2\text{KOH}(aq) + \text{H}_2(g) \) |
| 17 | Combustion | \( 2\text{C}_3\text{H}_{12}(l) + 21\text{O}_2(g) \rightarrow 12\text{H}_2\text{O}(g) + 6\text{CO}_2(g) \) |
| 18 | Double Displacement | \( 2\text{KOH}(aq) + \text{H}_2\text{CO}_3(aq) \rightarrow 2\text{H}_2\text{O}(l) + \text{K}_2\text{CO}_3(aq) \) |
| 19 | Combustion | \( 2\text{C}_4\text{H}_{10}(l) + 13\text{O}_2(g) \rightarrow 10\text{H}_2\text{O}(g) + 8\text{CO}_2(g) \) |
| 20 | Synthesis | \( 16\text{Al}(s) + 2\text{S}_8(s) \rightarrow 8\text{Al}_2\text{S}_3(s) \) |

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Final Answer

\[
\boxed{
\begin{array}{ll}
\text{1. } & \text{Zn}(s) + 2\text{AgNO}_3(aq) \rightarrow \text{Zn(NO}_3)_2(aq) + 2\text{Ag}(s) \\
\text{2. } & \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \\
\text{3. } & \text{NaCl}(aq) + \text{AgC}_2\text{H}_3\text{O}_2(aq) \rightarrow \text{NaC}_2\text{H}_3\text{O}_2(aq) + \text{AgCl}(s) \\
\text{4. } & 3\text{Mg(OH)}_2(aq) + 2\text{H}_3\text{PO}_4(aq) \rightarrow 6\text{H}_2\text{O}(l) + \text{Mg}_3(\text{PO}_4)_2(aq) \\
\text{5. } & 2\text{HNO}_3(aq) + \text{Ni}(s) \rightarrow \text{Ni(NO}_3)_2(aq) + \text{H}_2(g) \\
\text{6. } & \text{Ba(HCO}_3)_2(s) \rightarrow \text{BaCO}_3(s) + \text{H}_2\text{O}(g) + \text{CO}_2(g) \\
\text{7. } & \text{BaCl}_2(aq) + \text{Na}_2\text{SO}_4(aq) \rightarrow 2\text{NaCl}(aq) + \text{BaSO}_4(s) \\
\text{8. } & \text{Al}_2(\text{CO}_3)_3(s) \rightarrow \text{Al}_2\text{O}_3(s) + 3\text{CO}_2(g) \\
\text{9. } & \text{Ca}(s) + 2\text{H}_2\text{O}(l) \rightarrow \text{Ca(OH)}_2(aq) + \text{H}_2(g) \\
\text{10. } & 2\text{LiHCO}_3(s) \rightarrow \text{Li}_2\text{CO}_3(s) + \text{H}_2\text{O}(g) + \text{CO}_2(g) \\
\text{11. } & 2\text{N}_2(g) + 5\text{O}_2(g) \rightarrow 2\text{N}_2\text{O}_5(g) \\
\text{12. } & \text{MgBr}_2(aq) + 2\text{KOH}(aq) \rightarrow 2\text{KBr}(aq) + \text{Mg(OH)}_2(s) \\
\text{13. } & \text{Mn}(s) + \text{CuCl}_2(aq) \rightarrow \text{Cu}(s) + \text{MnCl}_2(s) \\
\text{14. } & 8\text{Zn}(s) + \text{S}_8(s) \rightarrow 8\text{ZnS}(s) \\
\text{15. } & 2\text{NaOH}(aq) + \text{H}_2\text{SO}_4(aq) \rightarrow 2\text{H}_2\text{O}(l) + \text{Na}_2\text{SO}_4(aq) \\
\text{16. } & 2\text{K}(s) + 2\text{H}_2\text{O}(l) \rightarrow 2\text{KOH}(aq) + \text{H}_2(g) \\
\text{17. } & 2\text{C}_3\text{H}_{12}(l) + 21\text{O}_2(g) \rightarrow 12\text{H}_2\text{O}(g) + 6\text{CO}_2(g) \\
\text{18. } & 2\text{KOH}(aq) + \text{H}_2\text{CO}_3(aq) \rightarrow 2\text{H}_2\text{O}(l) + \text{K}_2\text{CO}_3(aq) \\
\text{19. } & 2\text{C}_4\text{H}_{10}(l) + 13\text{O}_2(g) \rightarrow 10\text{H}_2\text{O}(g) + 8\text{CO}_2(g) \\
\text{20. } & 16\text{Al}(s) + 2\text{S}_8(s) \rightarrow 8\text{Al}_2\text{S}_3(s) \\
\end{array}
}
\]