Use the average bond enthalpies from Table 8.3 in your textbook to estimate AH for the formation of CO2(g) by the following reaction: CH4(g) + 202(g) --> CO2(g) +2H20(g) TABLE 8.3 Average Bond Enthalpies (kJ/mol) Single Bonds C-H 413 N-H 391 O-H 463 F-F 155 C-C 348 N-N 163 O-0 146 C-N 293 N-O 201 0-F 190 CI-F 253 C-o 358 N-F 272 0-CI 203 Cl-CI 242 C-F 485 N-CI 200 0-I 234 C-CI 328 N-Br 243 Br-F 237 C-Br 276 S-H 339 Br-CI 218 C-I 240 H-H 436 S-F 327 Br-Br 193 C-S 259 H-F 567 S-a 253 H-a 431 S-Br 218 I-a 208 S-H 323 H-B 366 S-S 266 I-Br 175 Si-SI 226 H-I 299 I-I 151 Si-C 301 Si-O 368 Si-Ca 464 Multiple Bonds C-C 614 N-N 418 495 CC 839 NN 941 C-N 615 N-o 607 S-0 523 C=N 891 S-S 418 C-o 799 Co 1072 +454 kJ/mol +763 kJ/mol -808 kJ/mol -201 kJ/mol 1911 kJ/mol O -1250 kJ/mol
Use the average bond enthalpies from Table 8.3 in your textbook to estimate AH for the formation of CO2(g) by the following reaction: CH4(g) + 202(g) --> CO2(g) +2H20(g) TABLE 8.3 Average Bond Enthalpies (kJ/mol) Single Bonds C-H 413 N-H 391 O-H 463 F-F 155 C-C 348 N-N 163 O-0 146 C-N 293 N-O 201 0-F 190 CI-F 253 C-o 358 N-F 272 0-CI 203 Cl-CI 242 C-F 485 N-CI 200 0-I 234 C-CI 328 N-Br 243 Br-F 237 C-Br 276 S-H 339 Br-CI 218 C-I 240 H-H 436 S-F 327 Br-Br 193 C-S 259 H-F 567 S-a 253 H-a 431 S-Br 218 I-a 208 S-H 323 H-B 366 S-S 266 I-Br 175 Si-SI 226 H-I 299 I-I 151 Si-C 301 Si-O 368 Si-Ca 464 Multiple Bonds C-C 614 N-N 418 495 CC 839 NN 941 C-N 615 N-o 607 S-0 523 C=N 891 S-S 418 C-o 799 Co 1072 +454 kJ/mol +763 kJ/mol -808 kJ/mol -201 kJ/mol 1911 kJ/mol O -1250 kJ/mol
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Chapter1: Chemical Foundations
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Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
![**Bond Enthalpy Estimation for CO₂ Formation**
Use the average bond enthalpies from Table 8.3 in your textbook to estimate the change in enthalpy (\( \Delta H \)) for the formation of CO₂(g) by the following reaction:
\[
\text{CH}_4(g) + 2\text{O}_2(g) \rightarrow \text{CO}_2(g) + 2\text{H}_2\text{O}(g)
\]
### Table 8.3: Average Bond Enthalpies (kJ/mol)
**Single Bonds**
- C–H: 413
- C–C: 348
- C–N: 293
- C–O: 358
- C–F: 485
- C–Cl: 328
- C–Br: 276
- N–N: 163
- N–O: 201
- N–F: 272
- N–Cl: 200
- N–Br: 243
- O–H: 463
- O–O: 146
- S–H: 339
- S–S: 266
- F–F: 155
- Cl–Cl: 242
**Multiple Bonds**
- C=C: 614
- C≡C: 839
- C=O: 799
- C≡O: 1072
- N=N: 418
### Multiple Choice Options for \( \Delta H \)
- +454 kJ/mol
- +763 kJ/mol
- -808 kJ/mol
- -201 kJ/mol
- 1911 kJ/mol
- -1250 kJ/mol
**Instructions:**
Using the bond enthalpy values provided, estimate the \( \Delta H \) for the reaction by calculating the total energy required to break all bonds in the reactants and the energy released in forming all bonds in the products. Select the correct answer from the options provided.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd523ae2e-d1e3-48cd-8a9c-04e15052448b%2F04d9db14-55ee-4022-a0b0-2c27b88dd8bc%2F9g0jcv_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Bond Enthalpy Estimation for CO₂ Formation**
Use the average bond enthalpies from Table 8.3 in your textbook to estimate the change in enthalpy (\( \Delta H \)) for the formation of CO₂(g) by the following reaction:
\[
\text{CH}_4(g) + 2\text{O}_2(g) \rightarrow \text{CO}_2(g) + 2\text{H}_2\text{O}(g)
\]
### Table 8.3: Average Bond Enthalpies (kJ/mol)
**Single Bonds**
- C–H: 413
- C–C: 348
- C–N: 293
- C–O: 358
- C–F: 485
- C–Cl: 328
- C–Br: 276
- N–N: 163
- N–O: 201
- N–F: 272
- N–Cl: 200
- N–Br: 243
- O–H: 463
- O–O: 146
- S–H: 339
- S–S: 266
- F–F: 155
- Cl–Cl: 242
**Multiple Bonds**
- C=C: 614
- C≡C: 839
- C=O: 799
- C≡O: 1072
- N=N: 418
### Multiple Choice Options for \( \Delta H \)
- +454 kJ/mol
- +763 kJ/mol
- -808 kJ/mol
- -201 kJ/mol
- 1911 kJ/mol
- -1250 kJ/mol
**Instructions:**
Using the bond enthalpy values provided, estimate the \( \Delta H \) for the reaction by calculating the total energy required to break all bonds in the reactants and the energy released in forming all bonds in the products. Select the correct answer from the options provided.
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