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Complete the table the theoretical o2 must be 23.25

To complete the table and ensure the theoretical O₂ requirement is 23.25 moles, we will need to determine the stoichiometric oxygen requirement for each component in the fuel mixture. Here's how we can approach this:

### Given Composition
We have the following components with their respective mole amounts in the feed basis of 100 moles:

- CO₂: 9.2 mol
- C₂H₄: 0.4 mol
- CO: 20.9 mol
- H₂: 15.6 mol
- CH₄: 1.9 mol
- N₂: 52 mol

### Steps to Complete the Table
1. **Calculate the total moles of Carbon (C), Hydrogen (H), and Oxygen (O) for each compound:**
   - **CO₂:** 1 C, 2 O per molecule
   - **C₂H₄:** 2 C, 4 H per molecule
   - **CO:** 1 C, 1 O per molecule
   - **H₂:** 2 H per molecule
   - **CH₄:** 1 C, 4 H per molecule
   - **N₂:** (No C, H, or O; inert gas)

2. **Compute the stoichiometric oxygen requirement (Theoretical O₂) for combustion:**
   - **CO₂:** No additional O₂ required as it’s already fully oxidized.
   - **C₂H₄:** Requires 3 O₂ for complete combustion to form CO₂ and H₂O.
   - **CO:** Requires 0.5 O₂ to convert each CO to CO₂.
   - **H₂:** Requires 0.5 O₂ to form H₂O.
   - **CH₄:** Requires 2 O₂ to form CO₂ and H₂O.

3. **Fill in the table values:**
   - **CO₂:** No O₂ needed (already oxidized).
   - **C₂H₄ (0.4 mol):** 0.4 * 3 = 1.2 mol O₂ required.
   - **CO (20.9 mol):** 20.9 * 0.5 = 10.45 mol O₂ required.
   - **H₂ (15.6 mol):** 15.6 * 0.5 = 7.8 mol O₂ required.
   - **CH₄ (1.9 mol):** 1.9 * 2 = 3.8 mol O₂ required.

Adding these up:
\[ \text{Total Theoretical O}_2 = 1.2 + 10.45 + 7.8 + 3.8 = 23.25 \, \text{moles} \]

### Table Completion

| Comp | Mol  | Total C | Total H | Total O | Total | Theo O₂ |
|------|------|---------|---------|---------|-------|---------|
| CO₂  | 9.2  | 9.2     | 0       | 18.4    | 9.2   | 0       |
| C₂H₄ | 0.4  | 0.8     | 1.6     | 0       | 0.4   | 1.2     |
| CO   | 20.9 | 20.9    | 0       | 20.9    | 20.9  | 10.45   |
| H₂   | 15.6 | 0       | 15.6    | 0       | 15.6  | 7.8     |
| CH₄  | 1.9  | 1.9     | 7.6     | 0       | 1.9   | 3.8     |
| N₂   | 52   | 0       | 0       | 0       | 52    | 0       |
| **Total** | **100** | **32.8** | **24.8** | **39.3** | **100** | **23.25** |

Would you like further details or have any questions about the calculations?

### Related Questions
1. How would you calculate the percent excess air for this combustion process?
2. What is the significance of using a "basis" of 100 moles in combustion calculations?
3. How does the presence of inert gases like N₂ affect the combustion process?
4. Why is it important to distinguish between dry and wet stack gas analyses?
5. How would changes in the feed composition affect the theoretical oxygen requirement?

### Tip
In combustion problems, always confirm that the theoretical oxygen aligns with the complete combustion of all hydrocarbons and carbon monoxide.

Complete the table with theoretical O₂ at 23.25 moles.

Learn to complete a combustion analysis table, calculating the theoretical O₂ requirement of 23.25 moles for a gaseous fuel composition. This problem involves stoichiometric and molar calculations, suitable for chemical engineering and chemistry students.

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