Two-column worksheet designed to help students practice naming reaction types and balancing the corresponding chemical equations.

Task: Identify Reaction Types and Balance Chemical Equations

The task involves two main steps:
1. Identify the type of chemical reaction for each equation.
2. Balance the chemical equations.

Below is the solution for each equation, including the reaction type and the balanced equation.

---

Step 1: Identify the type of chemical reaction

#### Reaction Types:
- Synthesis (Combination): Two or more substances combine to form one product.
- Decomposition: One substance breaks down into two or more simpler substances.
- Single Displacement: One element replaces another in a compound.
- Double Displacement (Precipitation/Acid-Base): Ions in two compounds exchange places to form two new compounds.
- Combustion: A substance reacts with oxygen to produce heat and light.
- Reduction-Oxidation (Redox): Involves the transfer of electrons between reactants.

---

Step 2: Balance the chemical equations

#### 1. Synthesis
$$
\text{N}_2 + \text{H}_2 \rightarrow \text{NH}_3
$$
- Reaction Type: Synthesis
- Balanced Equation:
$$
\text{N}_2 + 3\text{H}_2 \rightarrow 2\text{NH}_3
$$

#### 2. Decomposition
$$
\text{KClO}_3 \rightarrow \text{KCl} + \text{O}_2
$$
- Reaction Type: Decomposition
- Balanced Equation:
$$
2\text{KClO}_3 \rightarrow 2\text{KCl} + 3\text{O}_2
$$

#### 3. Single Displacement
$$
\text{NaCl} + \text{F}_2 \rightarrow \text{NaF} + \text{Cl}_2
$$
- Reaction Type: Single Displacement
- Balanced Equation:
$$
2\text{NaCl} + \text{F}_2 \rightarrow 2\text{NaF} + \text{Cl}_2
$$

#### 4. Synthesis
$$
\text{H}_2 + \text{O}_2 \rightarrow \text{H}_2\text{O}
$$
- Reaction Type: Synthesis
- Balanced Equation:
$$
2\text{H}_2 + \text{O}_2 \rightarrow 2\text{H}_2\text{O}
$$

#### 5. Double Displacement
$$
\text{AgNO}_3 + \text{MgCl}_2 \rightarrow \text{AgCl} + \text{Mg(NO}_3)_2
$$
- Reaction Type: Double Displacement
- Balanced Equation:
$$
2\text{AgNO}_3 + \text{MgCl}_2 \rightarrow 2\text{AgCl} + \text{Mg(NO}_3)_2
$$

#### 6. Double Displacement
$$
\text{AlBr}_3 + \text{K}_2\text{SO}_4 \rightarrow \text{KBr} + \text{Al}_2(\text{SO}_4)_3
$$
- Reaction Type: Double Displacement
- Balanced Equation:
$$
2\text{AlBr}_3 + 3\text{K}_2\text{SO}_4 \rightarrow 6\text{KBr} + \text{Al}_2(\text{SO}_4)_3
$$

#### 7. Combustion
$$
\text{CH}_4 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O}
$$
- Reaction Type: Combustion
- Balanced Equation:
$$
\text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O}
$$

#### 8. Combustion
$$
\text{C}_3\text{H}_8 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O}
$$
- Reaction Type: Combustion
- Balanced Equation:
$$
\text{C}_3\text{H}_8 + 5\text{O}_2 \rightarrow 3\text{CO}_2 + 4\text{H}_2\text{O}
$$

#### 9. Double Displacement
$$
\text{FeCl}_3 + \text{NaOH} \rightarrow \text{Fe(OH)}_3 + \text{NaCl}
$$
- Reaction Type: Double Displacement
- Balanced Equation:
$$
\text{FeCl}_3 + 3\text{NaOH} \rightarrow \text{Fe(OH)}_3 + 3\text{NaCl}
$$

#### 10. Synthesis
$$
\text{P} + \text{O}_2 \rightarrow \text{P}_2\text{O}_5
$$
- Reaction Type: Synthesis
- Balanced Equation:
$$
4\text{P} + 5\text{O}_2 \rightarrow 2\text{P}_2\text{O}_5
$$

#### 11. Single Displacement
$$
\text{Na} + \text{H}_2\text{O} \rightarrow \text{NaOH} + \text{H}_2
$$
- Reaction Type: Single Displacement
- Balanced Equation:
$$
2\text{Na} + 2\text{H}_2\text{O} \rightarrow 2\text{NaOH} + \text{H}_2
$$

#### 12. Decomposition
$$
\text{Ag}_2\text{O} \rightarrow \text{Ag} + \text{O}_2
$$
- Reaction Type: Decomposition
- Balanced Equation:
$$
2\text{Ag}_2\text{O} \rightarrow 4\text{Ag} + \text{O}_2
$$

#### 13. Photosynthesis
$$
\text{CO}_2 + \text{H}_2\text{O} \rightarrow \text{C}_6\text{H}_{12}\text{O}_6 + \text{O}_2
$$
- Reaction Type: Photosynthesis (Special Case of Synthesis)
- Balanced Equation:
$$
6\text{CO}_2 + 6\text{H}_2\text{O} \rightarrow \text{C}_6\text{H}_{12}\text{O}_6 + 6\text{O}_2
$$

#### 14. Single Displacement
$$
\text{K} + \text{MgBr}_2 \rightarrow \text{KBr} + \text{Mg}
$$
- Reaction Type: Single Displacement
- Balanced Equation:
$$
2\text{K} + \text{MgBr}_2 \rightarrow 2\text{KBr} + \text{Mg}
$$

#### 15. Double Displacement (Neutralization)
$$
\text{HNO}_3(aq) + \text{Ba(OH)}_2(aq) \rightarrow \text{Ba(NO}_3)_2(aq) + \text{H}_2\text{O}(l)
$$
- Reaction Type: Double Displacement (Neutralization)
- Balanced Equation:
$$
2\text{HNO}_3(aq) + \text{Ba(OH)}_2(aq) \rightarrow \text{Ba(NO}_3)_2(aq) + 2\text{H}_2\text{O}(l)
$$

#### 16. Combustion
$$
\text{C}_5\text{H}_{12}(g) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(g)
$$
- Reaction Type: Combustion
- Balanced Equation:
$$
\text{C}_5\text{H}_{12}(g) + 8\text{O}_2(g) \rightarrow 5\text{CO}_2(g) + 6\text{H}_2\text{O}(g)
$$

#### 17. Single Displacement
$$
\text{Al}(s) + \text{Fe}_2\text{O}_3(aq) \rightarrow \text{Al}_2\text{O}_3(aq) + \text{Fe}(s)
$$
- Reaction Type: Single Displacement
- Balanced Equation:
$$
2\text{Al}(s) + \text{Fe}_2\text{O}_3(aq) \rightarrow \text{Al}_2\text{O}_3(aq) + 2\text{Fe}(s)
$$

#### 18. Synthesis
$$
\text{Al}(s) + \text{O}_2(g) \rightarrow \text{Al}_2\text{O}_3(s)
$$
- Reaction Type: Synthesis
- Balanced Equation:
$$
4\text{Al}(s) + 3\text{O}_2(g) \rightarrow 2\text{Al}_2\text{O}_3(s)
$$

---

Final Answer:

$$
\boxed{
\begin{array}{ll}
1. & \text{N}_2 + 3\text{H}_2 \rightarrow 2\text{NH}_3 \\
2. & 2\text{KClO}_3 \rightarrow 2\text{KCl} + 3\text{O}_2 \\
3. & 2\text{NaCl} + \text{F}_2 \rightarrow 2\text{NaF} + \text{Cl}_2 \\
4. & 2\text{H}_2 + \text{O}_2 \rightarrow 2\text{H}_2\text{O} \\
5. & 2\text{AgNO}_3 + \text{MgCl}_2 \rightarrow 2\text{AgCl} + \text{Mg(NO}_3)_2 \\
6. & 2\text{AlBr}_3 + 3\text{K}_2\text{SO}_4 \rightarrow 6\text{KBr} + \text{Al}_2(\text{SO}_4)_3 \\
7. & \text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O} \\
8. & \text{C}_3\text{H}_8 + 5\text{O}_2 \rightarrow 3\text{CO}_2 + 4\text{H}_2\text{O} \\
9. & \text{FeCl}_3 + 3\text{NaOH} \rightarrow \text{Fe(OH)}_3 + 3\text{NaCl} \\
10. & 4\text{P} + 5\text{O}_2 \rightarrow 2\text{P}_2\text{O}_5 \\
11. & 2\text{Na} + 2\text{H}_2\text{O} \rightarrow 2\text{NaOH} + \text{H}_2 \\
12. & 2\text{Ag}_2\text{O} \rightarrow 4\text{Ag} + \text{O}_2 \\
13. & 6\text{CO}_2 + 6\text{H}_2\text{O} \rightarrow \text{C}_6\text{H}_{12}\text{O}_6 + 6\text{O}_2 \\
14. & 2\text{K} + \text{MgBr}_2 \rightarrow 2\text{KBr} + \text{Mg} \\
15. & 2\text{HNO}_3(aq) + \text{Ba(OH)}_2(aq) \rightarrow \text{Ba(NO}_3)_2(aq) + 2\text{H}_2\text{O}(l) \\
16. & \text{C}_5\text{H}_{12}(g) + 8\text{O}_2(g) \rightarrow 5\text{CO}_2(g) + 6\text{H}_2\text{O}(g) \\
17. & 2\text{Al}(s) + \text{Fe}_2\text{O}_3(aq) \rightarrow \text{Al}_2\text{O}_3(aq) + 2\text{Fe}(s) \\
18. & 4\text{Al}(s) + 3\text{O}_2(g) \rightarrow 2\text{Al}_2\text{O}_3(s) \\
\end{array}
}
$$