240 more combustion worksheets - Combustion Reactions Worksheet ... - Free Printable

Problem Overview:

The task is to write and balance the combustion reactions for various hydrocarbons and organic compounds, ensuring that the products are gaseous water (H₂O) and carbon dioxide (CO₂). Combustion reactions involve the reaction of a hydrocarbon or organic compound with oxygen gas (O₂) to produce CO₂ and H₂O.

General Approach:

1. Identify the reactants: The hydrocarbon or organic compound and oxygen gas (O₂).
2. Write the unbalanced equation: Start with the reactants on the left and the products (CO₂ and H₂O) on the right.
3. Balance the equation:
- Balance carbon atoms by adjusting the coefficients of CO₂.
- Balance hydrogen atoms by adjusting the coefficients of H₂O.
- Balance oxygen atoms by adjusting the coefficient of O₂.
4. Ensure all atoms are balanced: Double-check that the number of atoms of each element is the same on both sides of the equation.

Solutions:

#### 1. The combustion of methane gas:
Methane: \( \text{CH}_4 \)
- Reactants: \( \text{CH}_4 + \text{O}_2 \)
- Products: \( \text{CO}_2 + \text{H}_2\text{O} \)

Unbalanced: \( \text{CH}_4 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \)

- Balance carbon: 1 C atom in CH₄ → 1 CO₂.
- Balance hydrogen: 4 H atoms in CH₄ → 2 H₂O.
- Balance oxygen: 2 O atoms in O₂ → 2 O atoms in CO₂ + 1 O atom in H₂O (total 3 O atoms needed).

Final balanced equation:
\[ \text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O} \]

#### 2. The combustion of nonane gas:
Nonane: \( \text{C}_9\text{H}_{20} \)
- Reactants: \( \text{C}_9\text{H}_{20} + \text{O}_2 \)
- Products: \( \text{CO}_2 + \text{H}_2\text{O} \)

Unbalanced: \( \text{C}_9\text{H}_{20} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \)

- Balance carbon: 9 C atoms in C₉H₂₀ → 9 CO₂.
- Balance hydrogen: 20 H atoms in C₉H₂₀ → 10 H₂O.
- Balance oxygen: 2 O atoms in O₂ → 18 O atoms in 9 CO₂ + 10 O atoms in 10 H₂O (total 28 O atoms needed).

Final balanced equation:
\[ \text{C}_9\text{H}_{20} + 14\text{O}_2 \rightarrow 9\text{CO}_2 + 10\text{H}_2\text{O} \]

#### 3. The combustion of pentane gas:
Pentane: \( \text{C}_5\text{H}_{12} \)
- Reactants: \( \text{C}_5\text{H}_{12} + \text{O}_2 \)
- Products: \( \text{CO}_2 + \text{H}_2\text{O} \)

Unbalanced: \( \text{C}_5\text{H}_{12} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \)

- Balance carbon: 5 C atoms in C₅H₁₂ → 5 CO₂.
- Balance hydrogen: 12 H atoms in C₅H₁₂ → 6 H₂O.
- Balance oxygen: 2 O atoms in O₂ → 10 O atoms in 5 CO₂ + 6 O atoms in 6 H₂O (total 16 O atoms needed).

Final balanced equation:
\[ \text{C}_5\text{H}_{12} + 8\text{O}_2 \rightarrow 5\text{CO}_2 + 6\text{H}_2\text{O} \]

#### 4. The combustion of heptane gas:
Heptane: \( \text{C}_7\text{H}_{16} \)
- Reactants: \( \text{C}_7\text{H}_{16} + \text{O}_2 \)
- Products: \( \text{CO}_2 + \text{H}_2\text{O} \)

Unbalanced: \( \text{C}_7\text{H}_{16} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \)

- Balance carbon: 7 C atoms in C₇H₁₆ → 7 CO₂.
- Balance hydrogen: 16 H atoms in C₇H₁₆ → 8 H₂O.
- Balance oxygen: 2 O atoms in O₂ → 14 O atoms in 7 CO₂ + 8 O atoms in 8 H₂O (total 22 O atoms needed).

Final balanced equation:
\[ \text{C}_7\text{H}_{16} + 11\text{O}_2 \rightarrow 7\text{CO}_2 + 8\text{H}_2\text{O} \]

#### 5. The combustion of hexane gas:
Hexane: \( \text{C}_6\text{H}_{14} \)
- Reactants: \( \text{C}_6\text{H}_{14} + \text{O}_2 \)
- Products: \( \text{CO}_2 + \text{H}_2\text{O} \)

Unbalanced: \( \text{C}_6\text{H}_{14} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \)

- Balance carbon: 6 C atoms in C₆H₁₄ → 6 CO₂.
- Balance hydrogen: 14 H atoms in C₆H₁₄ → 7 H₂O.
- Balance oxygen: 2 O atoms in O₂ → 12 O atoms in 6 CO₂ + 7 O atoms in 7 H₂O (total 19 O atoms needed).

Final balanced equation:
\[ 2\text{C}_6\text{H}_{14} + 19\text{O}_2 \rightarrow 12\text{CO}_2 + 14\text{H}_2\text{O} \]

#### 6. The combustion of butane gas:
Butane: \( \text{C}_4\text{H}_{10} \)
- Reactants: \( \text{C}_4\text{H}_{10} + \text{O}_2 \)
- Products: \( \text{CO}_2 + \text{H}_2\text{O} \)

Unbalanced: \( \text{C}_4\text{H}_{10} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \)

- Balance carbon: 4 C atoms in C₄H₁₀ → 4 CO₂.
- Balance hydrogen: 10 H atoms in C₄H₁₀ → 5 H₂O.
- Balance oxygen: 2 O atoms in O₂ → 8 O atoms in 4 CO₂ + 5 O atoms in 5 H₂O (total 13 O atoms needed).

Final balanced equation:
\[ 2\text{C}_4\text{H}_{10} + 13\text{O}_2 \rightarrow 8\text{CO}_2 + 10\text{H}_2\text{O} \]

#### 7. The combustion of ethane gas:
Ethane: \( \text{C}_2\text{H}_6 \)
- Reactants: \( \text{C}_2\text{H}_6 + \text{O}_2 \)
- Products: \( \text{CO}_2 + \text{H}_2\text{O} \)

Unbalanced: \( \text{C}_2\text{H}_6 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \)

- Balance carbon: 2 C atoms in C₂H₆ → 2 CO₂.
- Balance hydrogen: 6 H atoms in C₂H₆ → 3 H₂O.
- Balance oxygen: 2 O atoms in O₂ → 4 O atoms in 2 CO₂ + 3 O atoms in 3 H₂O (total 7 O atoms needed).

Final balanced equation:
\[ 2\text{C}_2\text{H}_6 + 7\text{O}_2 \rightarrow 4\text{CO}_2 + 6\text{H}_2\text{O} \]

#### 8. The combustion of octane gas:
Octane: \( \text{C}_8\text{H}_{18} \)
- Reactants: \( \text{C}_8\text{H}_{18} + \text{O}_2 \)
- Products: \( \text{CO}_2 + \text{H}_2\text{O} \)

Unbalanced: \( \text{C}_8\text{H}_{18} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \)

- Balance carbon: 8 C atoms in C₈H₁₈ → 8 CO₂.
- Balance hydrogen: 18 H atoms in C₈H₁₈ → 9 H₂O.
- Balance oxygen: 2 O atoms in O₂ → 16 O atoms in 8 CO₂ + 9 O atoms in 9 H₂O (total 25 O atoms needed).

Final balanced equation:
\[ 2\text{C}_8\text{H}_{18} + 25\text{O}_2 \rightarrow 16\text{CO}_2 + 18\text{H}_2\text{O} \]

#### 9. The combustion of decane gas:
Decane: \( \text{C}_{10}\text{H}_{22} \)
- Reactants: \( \text{C}_{10}\text{H}_{22} + \text{O}_2 \)
- Products: \( \text{CO}_2 + \text{H}_2\text{O} \)

Unbalanced: \( \text{C}_{10}\text{H}_{22} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \)

- Balance carbon: 10 C atoms in C₁₀H₂₂ → 10 CO₂.
- Balance hydrogen: 22 H atoms in C₁₀H₂₂ → 11 H₂O.
- Balance oxygen: 2 O atoms in O₂ → 20 O atoms in 10 CO₂ + 11 O atoms in 11 H₂O (total 31 O atoms needed).

Final balanced equation:
\[ 2\text{C}_{10}\text{H}_{22} + 31\text{O}_2 \rightarrow 20\text{CO}_2 + 22\text{H}_2\text{O} \]

#### 10. The combustion of solid glucose (\( \text{C}_6\text{H}_{12}\text{O}_6 \)):
Glucose: \( \text{C}_6\text{H}_{12}\text{O}_6 \)
- Reactants: \( \text{C}_6\text{H}_{12}\text{O}_6 + \text{O}_2 \)
- Products: \( \text{CO}_2 + \text{H}_2\text{O} \)

Unbalanced: \( \text{C}_6\text{H}_{12}\text{O}_6 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \)

- Balance carbon: 6 C atoms in C₆H₁₂O₆ → 6 CO₂.
- Balance hydrogen: 12 H atoms in C₆H₁₂O₆ → 6 H₂O.
- Balance oxygen: 6 O atoms in C₆H₁₂O₆ → 6 O atoms in 6 CO₂ + 6 O atoms in 6 H₂O (total 12 O atoms needed).

Final balanced equation:
\[ \text{C}_6\text{H}_{12}\text{O}_6 + 6\text{O}_2 \rightarrow 6\text{CO}_2 + 6\text{H}_2\text{O} \]

#### 11. The combustion of sucrose (\( \text{C}_{12}\text{H}_{22}\text{O}_{11} \)):
Sucrose: \( \text{C}_{12}\text{H}_{22}\text{O}_{11} \)
- Reactants: \( \text{C}_{12}\text{H}_{22}\text{O}_{11} + \text{O}_2 \)
- Products: \( \text{CO}_2 + \text{H}_2\text{O} \)

Unbalanced: \( \text{C}_{12}\text{H}_{22}\text{O}_{11} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \)

- Balance carbon: 12 C atoms in C₁₂H₂₂O₁₁ → 12 CO₂.
- Balance hydrogen: 22 H atoms in C₁₂H₂₂O₁₁ → 11 H₂O.
- Balance oxygen: 11 O atoms in C₁₂H₂₂O₁₁ → 12 O atoms in 12 CO₂ + 11 O atoms in 11 H₂O (total 23 O atoms needed).

Final balanced equation:
\[ \text{C}_{12}\text{H}_{22}\text{O}_{11} + 12\text{O}_2 \rightarrow 12\text{CO}_2 + 11\text{H}_2\text{O} \]

Final Answer:

\[
\boxed{
\begin{aligned}
1. & \quad \text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O} \\
2. & \quad \text{C}_9\text{H}_{20} + 14\text{O}_2 \rightarrow 9\text{CO}_2 + 10\text{H}_2\text{O} \\
3. & \quad \text{C}_5\text{H}_{12} + 8\text{O}_2 \rightarrow 5\text{CO}_2 + 6\text{H}_2\text{O} \\
4. & \quad \text{C}_7\text{H}_{16} + 11\text{O}_2 \rightarrow 7\text{CO}_2 + 8\text{H}_2\text{O} \\
5. & \quad 2\text{C}_6\text{H}_{14} + 19\text{O}_2 \rightarrow 12\text{CO}_2 + 14\text{H}_2\text{O} \\
6. & \quad 2\text{C}_4\text{H}_{10} + 13\text{O}_2 \rightarrow 8\text{CO}_2 + 10\text{H}_2\text{O} \\
7. & \quad 2\text{C}_2\text{H}_6 + 7\text{O}_2 \rightarrow 4\text{CO}_2 + 6\text{H}_2\text{O} \\
8. & \quad 2\text{C}_8\text{H}_{18} + 25\text{O}_2 \rightarrow 16\text{CO}_2 + 18\text{H}_2\text{O} \\
9. & \quad 2\text{C}_{10}\text{H}_{22} + 31\text{O}_2 \rightarrow 20\text{CO}_2 + 22\text{H}_2\text{O} \\
10. & \quad \text{C}_6\text{H}_{12}\text{O}_6 + 6\text{O}_2 \rightarrow 6\text{CO}_2 + 6\text{H}_2\text{O} \\
11. & \quad \text{C}_{12}\text{H}_{22}\text{O}_{11} + 12\text{O}_2 \rightarrow 12\text{CO}_2 + 11\text{H}_2\text{O}
\end{aligned}
}
\]