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To complete the table and the analysis, let's break down the information given and fill in the missing values.

1. **Analyzing the Molecules:**
   - We have three hydrocarbons: **CH₄ (methane)**, **C₂H₆ (ethane)**, and **C₃H₈ (propane)**.
   - For each compound, we are given (or need to calculate) the moles and the total carbon (C) and hydrogen (H) atoms contributed by these compounds.

2. **Known Values:**
   - For CH₄:
     - Moles = 92
     - Total C = 92 (since each CH₄ molecule has 1 C atom)
     - Total H = 368 (since each CH₄ molecule has 4 H atoms)

3. **Calculating Values for C₂H₆ and C₃H₈:**
   - Let’s assume similar calculations for C₂H₆ and C₃H₈. 

Let’s go through the calculations.

### Calculation Steps

1. **For C₂H₆:**
   - If we assume **92 moles** of C₂H₆:
     - Total C = 92 * 2 = 184
     - Total H = 92 * 6 = 552

2. **For C₃H₈:**
   - If we assume **92 moles** of C₃H₈:
     - Total C = 92 * 3 = 276
     - Total H = 92 * 8 = 736

3. **Total Values for C and H:**
   - **Total C** = 92 (from CH₄) + 184 (from C₂H₆) + 276 (from C₃H₈) = 552
   - **Total H** = 368 (from CH₄) + 552 (from C₂H₆) + 736 (from C₃H₈) = 1656

### Filling in the Table

Based on these calculations, the table should look like this:

| Comp | Mol | Total C | Total H |
|------|-----|---------|---------|
| CH₄  | 92  | 92      | 368     |
| C₂H₆ | 92  | 184     | 552     |
| C₃H₈ | 92  | 276     | 736     |
| **Total** |   | **552** | **1656** |

### Theoretical Oxygen Requirement

To calculate the theoretical oxygen (\( \text{O}_2 \)) requirement for the combustion of these compounds, we consider that:
- Each C atom requires 1 molecule of \( \text{O}_2 \) for complete combustion to form \( \text{CO}_2 \).
- Each pair of H atoms requires 0.5 molecules of \( \text{O}_2 \) to form \( \text{H}_2\text{O} \).

#### Total Oxygen Calculation

1. For **C atoms**: \( 552 \) C atoms require \( 552 \) moles of \( \text{O}_2 \).
2. For **H atoms**: \( 1656 \) H atoms require \( \frac{1656}{2} = 828 \) moles of \( \text{O}_2 \).

**Total \( \text{O}_2 \) required** = 552 + 828 = 1380 moles

This calculation suggests a theoretical oxygen requirement of 1380 moles, differing from the 214.25 moles given, which might involve an additional factor or assumption not specified here. 

Would you like further details on these calculations, or do you have questions about any specific steps?

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Here are five related questions to explore further:
1. What are the complete balanced combustion equations for CH₄, C₂H₆, and C₃H₈?
2. How would the oxygen requirement change if we had different amounts of each hydrocarbon?
3. Why might the given theoretical oxygen (214.25 moles) differ from the calculated value?
4. How does the atomic method differ from a molecular approach in combustion calculations?
5. How would incomplete combustion affect the theoretical oxygen requirement?

**Tip:** Always double-check the mole ratios in stoichiometric calculations for accuracy, especially in combustion reactions.

Complete the table and determine the theoretical oxygen requirement for the combustion of methane (CH4), ethane (C2H6), and propane (C3H8) using atomic analysis.

Learn how to calculate the theoretical oxygen requirement for the combustion of methane (CH4), ethane (C2H6), and propane (C3H8) using atomic analysis. This problem involves stoichiometric calculations, mole conversions, and balanced chemical equations, making it suitable for undergraduate chemistry students.

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