Use the following table of bond energies to calculate the enthalpy of combustion (in kJ) of acetylene (C2H2) gas in oxygen, based on the following chemical equation: C2H2(g) + 2.502(g) → 2CO:(g) + H2O(g) Single H c|N |o Bond н 432 411 346 N 386 305 167 459 358 201 142 C=C 602 C=O 799 C=C 835 C=O 1072 Multiple Bonds C=N 615 O=0 494 C=N 887 N=N 942 **All values in kJ/mol**
Use the following table of bond energies to calculate the enthalpy of combustion (in kJ) of acetylene (C2H2) gas in oxygen, based on the following chemical equation: C2H2(g) + 2.502(g) → 2CO:(g) + H2O(g) Single H c|N |o Bond н 432 411 346 N 386 305 167 459 358 201 142 C=C 602 C=O 799 C=C 835 C=O 1072 Multiple Bonds C=N 615 O=0 494 C=N 887 N=N 942 **All values in kJ/mol**
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Use the following table of bond energies to calculate the enthalpy of combustion (in kJ) of acetylene (C₂H₂) gas in oxygen, based on the following chemical equation: C₂H₂(g) + 2.5O₂(g) → 2CO₂(g) + H₂O(g)
![**Title: Calculating the Enthalpy of Combustion of Acetylene**
To calculate the enthalpy of combustion (in kJ) of acetylene (C₂H₂) gas in oxygen, refer to the following chemical equation:
\[ \text{C}_2\text{H}_2(g) + 2.5\text{O}_2(g) \rightarrow 2\text{CO}_2(g) + \text{H}_2\text{O}(g) \]
**Bond Energies Table:**
The table below provides bond energies in kilojoules per mole (kJ/mol) for the bonds present in the reactants and products. These values will be used to calculate the total energy involved in breaking and forming bonds during the reaction.
| **Single Bond** | | H | C | N | O |
|-----------------|---|-----|-----|-----|-----|
| **H** | | 432 | | | |
| **C** | | 411 | 346 | | |
| **N** | | 386 | 305 | 167 | |
| **O** | | 459 | 358 | 201 | 142 |
| **Multiple Bonds** | |
|----------------------|---|
| C=C | 602 |
| C≡C | 835 |
| C=N | 615 |
| C≡N | 887 |
| C=O | 799 |
| C≡O | 1072 |
| O=O | 494 |
| N≡N | 942 |
*Note: All values are in kJ/mol.*
**Instructions for Use:**
1. Identify the bonds broken and formed in the chemical reaction.
2. Use the bond energies from the table to calculate the total energy required to break the bonds in the reactants.
3. Calculate the total energy released when new bonds are formed in the products.
4. Subtract the energy released from the energy required to obtain the enthalpy change (ΔH) for the reaction.
This approach allows for the estimation of the enthalpy of combustion of acetylene using standard bond energies.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc8a7502e-6db8-4a39-ada5-fdfb70d2ec95%2Fb13fc7af-6bed-4a84-82b5-425cb4ee0a4b%2F5lbstdt_processed.png&w=3840&q=75)
Transcribed Image Text:**Title: Calculating the Enthalpy of Combustion of Acetylene**
To calculate the enthalpy of combustion (in kJ) of acetylene (C₂H₂) gas in oxygen, refer to the following chemical equation:
\[ \text{C}_2\text{H}_2(g) + 2.5\text{O}_2(g) \rightarrow 2\text{CO}_2(g) + \text{H}_2\text{O}(g) \]
**Bond Energies Table:**
The table below provides bond energies in kilojoules per mole (kJ/mol) for the bonds present in the reactants and products. These values will be used to calculate the total energy involved in breaking and forming bonds during the reaction.
| **Single Bond** | | H | C | N | O |
|-----------------|---|-----|-----|-----|-----|
| **H** | | 432 | | | |
| **C** | | 411 | 346 | | |
| **N** | | 386 | 305 | 167 | |
| **O** | | 459 | 358 | 201 | 142 |
| **Multiple Bonds** | |
|----------------------|---|
| C=C | 602 |
| C≡C | 835 |
| C=N | 615 |
| C≡N | 887 |
| C=O | 799 |
| C≡O | 1072 |
| O=O | 494 |
| N≡N | 942 |
*Note: All values are in kJ/mol.*
**Instructions for Use:**
1. Identify the bonds broken and formed in the chemical reaction.
2. Use the bond energies from the table to calculate the total energy required to break the bonds in the reactants.
3. Calculate the total energy released when new bonds are formed in the products.
4. Subtract the energy released from the energy required to obtain the enthalpy change (ΔH) for the reaction.
This approach allows for the estimation of the enthalpy of combustion of acetylene using standard bond energies.
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