Classifying Chemical Reactions Worksheet | Exercises Chemistry ... - Free Printable

To solve this worksheet, we need to look at the pattern of each chemical equation and match it to the definitions of the reaction types provided in the instructions: acid/base, redox, synthesis, decomposition, single replacement, double replacement, or combustion.

Here is the step-by-step breakdown for each reaction:

1. PbCl₂ + AgNO₃ → Pb(NO₃)₂ + AgCl
* Analysis: Two ionic compounds swap partners. Lead (Pb) pairs with Nitrate (NO₃), and Silver (Ag) pairs with Chloride (Cl).
* Type: Double Replacement.

2. NH₃ + HCl → NH₄Cl
* Analysis: Ammonia (NH₃) acts as a base and Hydrochloric acid (HCl) acts as an acid. They combine to form a salt (Ammonium chloride).
* Type: Acid/Base. (Note: It is also a Synthesis reaction, but Acid/Base is the specific chemical interaction here).

3. AlCl₃ + Na₂SO₄ → Al₂(SO₄)₃ + NaCl
* Analysis: Aluminum (Al) swaps with Sodium (Na). The cations switch places.
* Type: Double Replacement.

4. Zn + S → ZnS
* Analysis: Two elements (Zinc and Sulfur) combine to form a single compound.
* Type: Synthesis. (Note: This is also Redox because oxidation states change, but Synthesis is the structural pattern).

5. Al₂(SO₄)₃ + BaCl₂ → BaSO₄ + AlCl₃
* Analysis: Aluminum (Al) swaps with Barium (Ba).
* Type: Double Replacement.

6. Al₂S₃ → Al + S
* Analysis: A single compound breaks down into simpler substances (elements).
* Type: Decomposition. (Note: This is also Redox).

7. H₂SO₄ + Fe → H₂ + FeSO₄
* Analysis: Iron (Fe), an element, replaces Hydrogen (H) in the compound Sulfuric Acid.
* Type: Single Replacement. (Note: This is also Redox and Acid/Metal reaction).

8. C₁₂H₂₂O₁₁ + O₂ → CO₂ + H₂O
* Analysis: A hydrocarbon/carbohydrate reacts with Oxygen to produce Carbon Dioxide and Water.
* Type: Combustion. (Note: This is also Redox).

9. Mg(OH)₂ + H₂SO₄ → MgSO₄ + H₂O
* Analysis: Magnesium Hydroxide (Base) reacts with Sulfuric Acid to form a salt and water.
* Type: Acid/Base. (Also Double Replacement).

10. NaOH + CuSO₄ → Na₂SO₄ + Cu(OH)₂
* Analysis: Sodium (Na) swaps with Copper (Cu).
* Type: Double Replacement.

11. C₄H₁₂ + O₂ → H₂O + CO₂
* Analysis: A hydrocarbon reacts with Oxygen to produce CO₂ and H₂O.
* Type: Combustion. (Note: The formula C4H12 is chemically impossible for a standard hydrocarbon, but the pattern clearly indicates combustion).

12. Fe + O₂ → Fe₂O₃
* Analysis: Iron combines with Oxygen to form a single compound (Rust).
* Type: Synthesis. (Also Redox).

13. Mg₃(PO₄)₂ + H₂ → Mg + H₃PO₄
* Analysis: Hydrogen (H) replaces Magnesium (Mg) in the phosphate compound.
* Type: Single Replacement. (Also Redox).

14. NH₄NO₃ → N₂O + H₂O
* Analysis: One reactant breaks down into two products.
* Type: Decomposition. (Also Redox).

15. Cl₂ + KBr → KCl + Br₂
* Analysis: Chlorine (Cl), an element, replaces Bromine (Br) in the compound.
* Type: Single Replacement. (Also Redox).

Final Answer:
1. Double Replacement
2. Acid/Base
3. Double Replacement
4. Synthesis
5. Double Replacement
6. Decomposition
7. Single Replacement
8. Combustion
9. Acid/Base
10. Double Replacement
11. Combustion
12. Synthesis
13. Single Replacement
14. Decomposition
15. Single Replacement