Calculate the heat of reaction AH for the following reaction: 2 CH₂(g) + 30₂(g) →2 CO(g) + 4H₂O(g) You can find a table of bond energies by using the Data button on the ALEKS toolbar. Round your answer to the nearest kJ/mol. kJ mol olo Data bond H-H H-F H-CI H-Br H-I H-C H-O H-N H-P H-S bond C-H C-F C-CI C-Br energy (kJ/mol) 436 570 431 366 298 413 497 391 351 381 energy (kJ/mol) 413 460 350 293 bond O-H O-F O-CI O-Br O-I O-C O=C O=C O-O O=O O-N O=N O=S bond N-H N-C N=C N=C energy (kJ/mol) 497 215 234 210 213 385 532 1077 210 498 206 631 551 energy (kJ/mol) 391 356 615 749 bond F-F F-CI F-Br F-I CI-CI Cl-Br CI-I Br-Br Br-I I-I bond S-H S-F S-CI S-Br energy (kJ/mol) 159 261 280 272 243 219 211 194 179 152 energy (kJ/mol) 381 392 272 230
Calculate the heat of reaction AH for the following reaction: 2 CH₂(g) + 30₂(g) →2 CO(g) + 4H₂O(g) You can find a table of bond energies by using the Data button on the ALEKS toolbar. Round your answer to the nearest kJ/mol. kJ mol olo Data bond H-H H-F H-CI H-Br H-I H-C H-O H-N H-P H-S bond C-H C-F C-CI C-Br energy (kJ/mol) 436 570 431 366 298 413 497 391 351 381 energy (kJ/mol) 413 460 350 293 bond O-H O-F O-CI O-Br O-I O-C O=C O=C O-O O=O O-N O=N O=S bond N-H N-C N=C N=C energy (kJ/mol) 497 215 234 210 213 385 532 1077 210 498 206 631 551 energy (kJ/mol) 391 356 615 749 bond F-F F-CI F-Br F-I CI-CI Cl-Br CI-I Br-Br Br-I I-I bond S-H S-F S-CI S-Br energy (kJ/mol) 159 261 280 272 243 219 211 194 179 152 energy (kJ/mol) 381 392 272 230
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
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
![### Calculating the Heat of Reaction (ΔH)
**Reaction:**
\[ 2 \text{CH}_4(g) + 3 \text{O}_2(g) \rightarrow 2 \text{CO}(g) + 4 \text{H}_2\text{O}(g) \]
To find the heat of reaction, you use bond energies provided in the following table.
**Bond Energy Data Table**
This table lists various chemical bonds and their corresponding bond energy values in kilojoules per mole (kJ/mol):
- **Hydrogen Bonds:**
- H-H: 436
- H-F: 570
- H-Cl: 431
- H-Br: 366
- H-I: 298
- H-C: 413
- H-O: 497
- H-N: 391
- H-P: 351
- H-S: 381
- **Oxygen Bonds:**
- O-H: 497
- O-F: 215
- O-Cl: 234
- O-Br: 210
- O-I: 213
- O-C: 385
- O=C: 532
- O≡C: 1077
- O-O: 210
- O=O: 498
- O=N: 631
- O=S: 551
- **Fluorine Bonds:**
- F-F: 159
- F-Cl: 261
- F-Br: 280
- F-I: 272
- **Chlorine Bonds:**
- Cl-Cl: 243
- Cl-Br: 219
- Cl-I: 211
- **Bromine Bonds:**
- Br-Br: 194
- Br-I: 179
- **Iodine Bonds:**
- I-I: 152
- **Carbon Bonds:**
- C-H: 413
- C-F: 460
- C-Cl: 350
- C-Br: 293
- **Nitrogen Bonds:**
- N-H: 391
- N-C: 356
- N≡C: 615
- N≡C: 749](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d7adbf1-3ca3-4012-a27a-9468e79345de%2F1319788c-9c6a-47d7-be09-b801762c6aff%2Fv5ir6na_processed.png&w=3840&q=75)
Transcribed Image Text:### Calculating the Heat of Reaction (ΔH)
**Reaction:**
\[ 2 \text{CH}_4(g) + 3 \text{O}_2(g) \rightarrow 2 \text{CO}(g) + 4 \text{H}_2\text{O}(g) \]
To find the heat of reaction, you use bond energies provided in the following table.
**Bond Energy Data Table**
This table lists various chemical bonds and their corresponding bond energy values in kilojoules per mole (kJ/mol):
- **Hydrogen Bonds:**
- H-H: 436
- H-F: 570
- H-Cl: 431
- H-Br: 366
- H-I: 298
- H-C: 413
- H-O: 497
- H-N: 391
- H-P: 351
- H-S: 381
- **Oxygen Bonds:**
- O-H: 497
- O-F: 215
- O-Cl: 234
- O-Br: 210
- O-I: 213
- O-C: 385
- O=C: 532
- O≡C: 1077
- O-O: 210
- O=O: 498
- O=N: 631
- O=S: 551
- **Fluorine Bonds:**
- F-F: 159
- F-Cl: 261
- F-Br: 280
- F-I: 272
- **Chlorine Bonds:**
- Cl-Cl: 243
- Cl-Br: 219
- Cl-I: 211
- **Bromine Bonds:**
- Br-Br: 194
- Br-I: 179
- **Iodine Bonds:**
- I-I: 152
- **Carbon Bonds:**
- C-H: 413
- C-F: 460
- C-Cl: 350
- C-Br: 293
- **Nitrogen Bonds:**
- N-H: 391
- N-C: 356
- N≡C: 615
- N≡C: 749
![**Calculating the Heat of Reaction (ΔH) for a Chemical Reaction**
**Reaction:**
\[ 2 \text{CH}_4(g) + 3 \text{O}_2(g) \rightarrow 2 \text{CO}(g) + 4 \text{H}_2\text{O}(g) \]
**Instructions:**
Calculate the heat of reaction \(\Delta H\) for the given equation by using the provided bond energy data. Round your answer to the nearest kJ/mol.
**Bond Energy Data Table:**
This table lists various types of chemical bonds and their corresponding bond energies in kilojoules per mole (kJ/mol).
- **Column 1:**
- **C-H:** 413
- **C-F:** 460
- **C-Cl:** 350
- **C-Br:** 293
- **C-I:** 211
- **C-C:** 370
- **C=C:** 602
- **C≡C:** 839
- **C-O:** 385
- **C=O:** 532
- **C≡O:** 1077
- **C-N:** 356
- **C=N:** 615
- **C≡N:** 749
- **C-P:** 263
- **C-S:** 312
- **C=S:** 397
- **C-Si:** 375
- **Column 2:**
- **N-H:** 391
- **N-C:** 356
- **N≡C:** 615
- **N≡C:** 749
- **N-O:** 206
- **N=O:** 631
- **N≡O:** 1020
- **N=N:** 277
- **N≡N:** 418
- **N≡N:** 945
- **N-P:** 209
- **N-F:** 349
- **N-Cl:** 334
- **N-Br:** 281
- **Column 3:**
- **S-H:** 381
- **S-F:** 392
- **S-Cl:** 272
- **](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d7adbf1-3ca3-4012-a27a-9468e79345de%2F1319788c-9c6a-47d7-be09-b801762c6aff%2Fol8vg2_processed.png&w=3840&q=75)
Transcribed Image Text:**Calculating the Heat of Reaction (ΔH) for a Chemical Reaction**
**Reaction:**
\[ 2 \text{CH}_4(g) + 3 \text{O}_2(g) \rightarrow 2 \text{CO}(g) + 4 \text{H}_2\text{O}(g) \]
**Instructions:**
Calculate the heat of reaction \(\Delta H\) for the given equation by using the provided bond energy data. Round your answer to the nearest kJ/mol.
**Bond Energy Data Table:**
This table lists various types of chemical bonds and their corresponding bond energies in kilojoules per mole (kJ/mol).
- **Column 1:**
- **C-H:** 413
- **C-F:** 460
- **C-Cl:** 350
- **C-Br:** 293
- **C-I:** 211
- **C-C:** 370
- **C=C:** 602
- **C≡C:** 839
- **C-O:** 385
- **C=O:** 532
- **C≡O:** 1077
- **C-N:** 356
- **C=N:** 615
- **C≡N:** 749
- **C-P:** 263
- **C-S:** 312
- **C=S:** 397
- **C-Si:** 375
- **Column 2:**
- **N-H:** 391
- **N-C:** 356
- **N≡C:** 615
- **N≡C:** 749
- **N-O:** 206
- **N=O:** 631
- **N≡O:** 1020
- **N=N:** 277
- **N≡N:** 418
- **N≡N:** 945
- **N-P:** 209
- **N-F:** 349
- **N-Cl:** 334
- **N-Br:** 281
- **Column 3:**
- **S-H:** 381
- **S-F:** 392
- **S-Cl:** 272
- **
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