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To solve this problem, we need to determine the energy produced when 225 g of \( \text{C}_2\text{H}_2 \) is burned, based on the provided enthalpy change for the reaction.

### Step-by-Step Solution

1. **Convert grams of \( \text{C}_2\text{H}_2 \) to moles:**
   \[
   \text{Molar mass of } \text{C}_2\text{H}_2 = 26.04 \, \text{g/mol}
   \]
   \[
   \text{Moles of } \text{C}_2\text{H}_2 = \frac{225 \, \text{g}}{26.04 \, \text{g/mol}} \approx 8.64 \, \text{mol}
   \]

2. **Use the reaction's enthalpy to find the energy produced:**
   According to the balanced chemical equation:
   \[
   2 \, \text{mol} \, \text{C}_2\text{H}_2 \rightarrow \text{produces} \, 2600 \, \text{kJ}
   \]
   
   To find the energy produced by 8.64 mol of \( \text{C}_2\text{H}_2 \), set up a proportion:
   \[
   \frac{2600 \, \text{kJ}}{2 \, \text{mol}} = X \, \text{kJ from 8.64 mol}
   \]
   Solving for \( X \):
   \[
   X = 8.64 \, \text{mol} \times \frac{2600 \, \text{kJ}}{2 \, \text{mol}} = 8.64 \times 1300 = 11232 \, \text{kJ}
   \]

### Answer
The energy produced is \( 1.12 \times 10^4 \, \text{kJ} \).

### Correct Option
The correct answer is:
- **\( 1.12 \times 10^4 \, \text{kJ} \)**

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#### Related Questions
1. How would the energy change if 300 g of \( \text{C}_2\text{H}_2 \) were burned?
2. What would happen to the energy produced if only 1 mol of \( \text{C}_2\text{H}_2 \) were used?
3. If the enthalpy change were different, say \(-5200 \, \text{kJ}\), how would that affect the answer?
4. How does stoichiometry help determine energy production in reactions like this?
5. Why do we ignore the negative sign in this energy calculation?

#### Tip
In stoichiometry problems involving energy, always check if the reaction is balanced and identify the correct molar ratios for conversions.

How much energy is produced when 225 g of C2H2 (26.04) is burned in excess O2?

Learn to calculate the energy produced when 225 g of C2H2 combusts in excess O2 using stoichiometry and thermochemical equations. This step-by-step solution covers key concepts in energy calculations, mole conversions, and balanced chemical reactions, suitable for high school chemistry students in Grades 10-12.

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