https://file.aiquickdraw.com/mathbot/file/17287121483596xqt2erv.jpg

Let's balance both of the combustion reactions in the image.

### 1. First reaction: 
\[
C_7H_{16} + O_2 \rightarrow H_2O(l) + CO_2(g)
\]

#### Step-by-step balancing:
1. **Balance carbon atoms (C)**:
   - On the left, we have 7 carbon atoms from \( C_7H_{16} \).
   - On the right, we need 7 carbon dioxide molecules to balance the carbon: 
     \[
     C_7H_{16} + O_2 \rightarrow H_2O + 7CO_2
     \]

2. **Balance hydrogen atoms (H)**:
   - On the left, there are 16 hydrogen atoms from \( C_7H_{16} \).
   - To balance, we need 8 water molecules (each water molecule contributes 2 hydrogen atoms):
     \[
     C_7H_{16} + O_2 \rightarrow 8H_2O + 7CO_2
     \]

3. **Balance oxygen atoms (O)**:
   - On the right side, we now have \( 8 \times 1 = 8 \) oxygen atoms from water and \( 7 \times 2 = 14 \) oxygen atoms from carbon dioxide, giving a total of \( 8 + 14 = 22 \) oxygen atoms.
   - To get 22 oxygen atoms on the left side, we need 11 \( O_2 \) molecules:
     \[
     C_7H_{16} + 11O_2 \rightarrow 8H_2O + 7CO_2
     \]

Thus, the balanced equation is:
\[
C_7H_{16} + 11O_2 \rightarrow 8H_2O + 7CO_2
\]

---

### 2. Second reaction:
\[
C_4H_8 + O_2 \rightarrow H_2O(l) + CO_2(g)
\]

#### Step-by-step balancing:
1. **Balance carbon atoms (C)**:
   - On the left, we have 4 carbon atoms from \( C_4H_8 \).
   - On the right, we need 4 carbon dioxide molecules:
     \[
     C_4H_8 + O_2 \rightarrow H_2O + 4CO_2
     \]

2. **Balance hydrogen atoms (H)**:
   - On the left, we have 8 hydrogen atoms from \( C_4H_8 \).
   - To balance, we need 4 water molecules:
     \[
     C_4H_8 + O_2 \rightarrow 4H_2O + 4CO_2
     \]

3. **Balance oxygen atoms (O)**:
   - On the right side, we now have \( 4 \times 1 = 4 \) oxygen atoms from water and \( 4 \times 2 = 8 \) oxygen atoms from carbon dioxide, giving a total of \( 4 + 8 = 12 \) oxygen atoms.
   - To get 12 oxygen atoms on the left side, we need 6 \( O_2 \) molecules:
     \[
     C_4H_8 + 6O_2 \rightarrow 4H_2O + 4CO_2
     \]

Thus, the balanced equation is:
\[
C_4H_8 + 6O_2 \rightarrow 4H_2O + 4CO_2
\]

---

Would you like further explanation on any of the steps?

### Related questions:
1. How do you balance equations involving polyatomic ions?
2. What are the types of reactions where combustion plays a role?
3. Why is balancing oxygen typically done last in combustion reactions?
4. How do stoichiometric coefficients relate to mole ratios in balanced equations?
5. Can combustion reactions occur without oxygen?

#### Tip:
When balancing chemical equations, it often helps to leave oxygen until the end, especially in combustion reactions, as it appears in multiple compounds.

Learn how to balance the combustion reactions of C_7H_{16} and C_4H_8 with step-by-step solutions. This problem involves stoichiometry, the law of conservation of mass, and the principles of chemical equation balancing. Suitable for high school chemistry students.

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