Using some of the bond energies, calculate AH(in kJ) for the following reaction: CH4 (g) + 202(g) → CO2(g) + 2H₂O(g) You will need to draw the Lewis Structure for the reactant and product molecules to determine which bond energy values to use. C=C 614 kJ/mol O-H 467 kJ/mol C-H= 413 kJ/mol C=C= 839 kJ/mol O-O 204 kJ/mol O=O= 498 kJ/mol C=O=799 kJ/mol C-C = 347 kJ/mol
Using some of the bond energies, calculate AH(in kJ) for the following reaction: CH4 (g) + 202(g) → CO2(g) + 2H₂O(g) You will need to draw the Lewis Structure for the reactant and product molecules to determine which bond energy values to use. C=C 614 kJ/mol O-H 467 kJ/mol C-H= 413 kJ/mol C=C= 839 kJ/mol O-O 204 kJ/mol O=O= 498 kJ/mol C=O=799 kJ/mol C-C = 347 kJ/mol
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ISBN:9781285199047
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Chapter16: Thermodynamics: Directionality Of Chemical Reactions
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![### Calculating ΔH for a Chemical Reaction
**Objective:** Using some of the bond energies, calculate ΔH (in kJ) for the following reaction:
\[ \text{CH}_4 \text{ (g)} + 2\text{O}_2 \text{ (g)} \rightarrow \text{CO}_2 \text{ (g)} + 2\text{H}_2\text{O} \text{ (g)} \]
You will need to draw the Lewis Structure for the reactant and product molecules to determine which bond energy values to use.
#### Bond Energies
- C=C = 614 kJ/mol
- O-H = 467 kJ/mol
- C-H = 413 kJ/mol
- C≡C = 839 kJ/mol
- O=O = 204 kJ/mol
- O=O = 498 kJ/mol
- C=O = 799 kJ/mol
- C-C = 347 kJ/mol
#### Steps for Calculation
1. **Draw the Lewis Structures** for each molecule in the reaction to identify the types and numbers of bonds.
2. **Calculate the total bond energy** for bonds broken in the reactants.
3. **Calculate the total bond energy** for bonds formed in the products.
4. **Subtract the bond energies of the products from the bond energies of the reactants** to find the overall ΔH:
\[ \Delta H = \Sigma \text{Bond Energies of Reactants} - \Sigma \text{Bond Energies of Products} \]
#### Example Calculation
**Reactants:**
- **CH4**: 4 C-H bonds
- **2 O2**: 2 O=O bonds
**Products:**
- **CO2**: 2 C=O bonds
- **2 H2O**: 4 O-H bonds
### Bond Energies in the Reaction
- **Reactants:**
- C-H: 4 × 413 = 1652 kJ/mol
- O=O: 2 × 498 = 996 kJ/mol
- Total bond energy for reactants = 1652 + 996 = 2648 kJ/mol
- **Products:**
- C=O: 2 × 799 = 1598 kJ/mol
- O-H: 4](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0a6c9e0c-0b6a-4785-ae3f-5e292bd65bb9%2F2a033a71-1b20-4fa6-b30a-7842cc49af81%2F0sw5esf_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Calculating ΔH for a Chemical Reaction
**Objective:** Using some of the bond energies, calculate ΔH (in kJ) for the following reaction:
\[ \text{CH}_4 \text{ (g)} + 2\text{O}_2 \text{ (g)} \rightarrow \text{CO}_2 \text{ (g)} + 2\text{H}_2\text{O} \text{ (g)} \]
You will need to draw the Lewis Structure for the reactant and product molecules to determine which bond energy values to use.
#### Bond Energies
- C=C = 614 kJ/mol
- O-H = 467 kJ/mol
- C-H = 413 kJ/mol
- C≡C = 839 kJ/mol
- O=O = 204 kJ/mol
- O=O = 498 kJ/mol
- C=O = 799 kJ/mol
- C-C = 347 kJ/mol
#### Steps for Calculation
1. **Draw the Lewis Structures** for each molecule in the reaction to identify the types and numbers of bonds.
2. **Calculate the total bond energy** for bonds broken in the reactants.
3. **Calculate the total bond energy** for bonds formed in the products.
4. **Subtract the bond energies of the products from the bond energies of the reactants** to find the overall ΔH:
\[ \Delta H = \Sigma \text{Bond Energies of Reactants} - \Sigma \text{Bond Energies of Products} \]
#### Example Calculation
**Reactants:**
- **CH4**: 4 C-H bonds
- **2 O2**: 2 O=O bonds
**Products:**
- **CO2**: 2 C=O bonds
- **2 H2O**: 4 O-H bonds
### Bond Energies in the Reaction
- **Reactants:**
- C-H: 4 × 413 = 1652 kJ/mol
- O=O: 2 × 498 = 996 kJ/mol
- Total bond energy for reactants = 1652 + 996 = 2648 kJ/mol
- **Products:**
- C=O: 2 × 799 = 1598 kJ/mol
- O-H: 4
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