### Understanding Bond Enthalpies**Use bond enthalpies in the table below to estimate ΔH for each of the following reactions.**#### Average Bond Enthalpies (kJ/mol)| Bond | Enthalpy (kJ/mol) | Bond | Enthalpy (kJ/mol) | Bond | Enthalpy (kJ/mol) ||------|-------------------|------|-------------------|------|-------------------|| C–H | 413 | N–H | 391 | O–H | 463 || C≡C | 848 | N–N | 163 | O=O | 146 || C=C | 614 | N≡N | 201 | O=O | 495 || C=O | 799 | Cl–Cl| 243 | O–O | 146 || C≡N | 891 | Cl–F | 253 | O–Cl | 203 || C–Cl | 328 | H–F | 567 | I–Cl | 208 || C–Br | 276 | H–Cl | 431 | I–Br | 175 || C–I | 240 | H–Br | 366 | I–I | 151 || H–I | 299 | H–O | 463 | Br–Br| 193 |### Example Reaction**Part A:**Reactants: ![bromomethane](https://www.example.com/br-c-h) and chlorine (![Cl\_2](https://www.example.com/Cl\_2))Products: ![dibromomethane](https://www.example.com/br-br), hydrogen chloride (![HCl](https://www.example.com/HCl))Product Diagram: Br-C-H + Cl-Cl -> Br-C-Cl + H-Cl**Express your answer in kilojoules to three significant figures.**ΔH = -202.3 kJ(Correct answer not provided)### Graph Explanation**Part B:**Reactants: ethane (![C_2H_2](https://www.example.com/C_2H_2))

∆Hreaction = ∑Bond energy of reactants ‒ ∑Bond energy of products

Use bond enthalpies in the table below to estimate AH for each of the following reactions. I Review Constants Periodic Table Part A Average bond enthalpy (kJ/mol) C-H: 413 N-H: 391 O-H: 463 F-F: 155 Br Br C-C: 348 N-N: 163 O-0: 146 Br-C-H + Cl-Cl - Br-C-Cl + Cl-H C=C: 614 N-O: 201 0=0: 495 Cl-F: 253 C-N: 293 N-F: 272 0-F: 190 Cl-Cl: 242 Br Br C-0: 358 N-Cl: 200 O-Cl: 203 Br-F: 237 234 Br-Cl: 218 Br-Br: 193 C=0: 799 N-Br: 243 0-I: Express your answer in kilojoules to three significant figures. C-F: 485 H-H: 436 C-Cl: 328 H-F: 567 C-Br: 276 H-Cl: 431 I-Cl: 208 kJ 202.3 240 H-Br: 366 H-I: 299 I-Br: 175 ΔΗ- C-I: I-I: 151 Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Part B H. H-C-H +2 0=0- 0=C=0+ 2 H-O-H

Use bond enthalpies in the table below to estimate AH for each of the following reactions. I Review Constants Periodic Table Part A Average bond enthalpy (kJ/mol) C-H: 413 N-H: 391 O-H: 463 F-F: 155 Br Br C-C: 348 N-N: 163 O-0: 146 Br-C-H + Cl-Cl - Br-C-Cl + Cl-H C=C: 614 N-O: 201 0=0: 495 Cl-F: 253 C-N: 293 N-F: 272 0-F: 190 Cl-Cl: 242 Br Br C-0: 358 N-Cl: 200 O-Cl: 203 Br-F: 237 234 Br-Cl: 218 Br-Br: 193 C=0: 799 N-Br: 243 0-I: Express your answer in kilojoules to three significant figures. C-F: 485 H-H: 436 C-Cl: 328 H-F: 567 C-Br: 276 H-Cl: 431 I-Cl: 208 kJ 202.3 240 H-Br: 366 H-I: 299 I-Br: 175 ΔΗ- C-I: I-I: 151 Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Part B H. H-C-H +2 0=0- 0=C=0+ 2 H-O-H

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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Concept explainers

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

### Understanding Bond Enthalpies

**Use bond enthalpies in the table below to estimate ΔH for each of the following reactions.**

#### Average Bond Enthalpies (kJ/mol)
| Bond | Enthalpy (kJ/mol) | Bond | Enthalpy (kJ/mol) | Bond | Enthalpy (kJ/mol) |
|------|-------------------|------|-------------------|------|-------------------|
| C–H | 413 | N–H | 391 | O–H | 463 |
| C≡C | 848 | N–N | 163 | O=O | 146 |
| C=C | 614 | N≡N | 201 | O=O | 495 |
| C=O | 799 | Cl–Cl| 243 | O–O | 146 |
| C≡N | 891 | Cl–F | 253 | O–Cl | 203 |
| C–Cl | 328 | H–F | 567 | I–Cl | 208 |
| C–Br | 276 | H–Cl | 431 | I–Br | 175 |
| C–I | 240 | H–Br | 366 | I–I | 151 |
| H–I | 299 | H–O | 463 | Br–Br| 193 |

### Example Reaction

**Part A:**

Reactants: ![bromomethane](https://www.example.com/br-c-h) and chlorine (![Cl\_2](https://www.example.com/Cl\_2))

Products: ![dibromomethane](https://www.example.com/br-br), hydrogen chloride (![HCl](https://www.example.com/HCl))

Product Diagram:
Br-C-H + Cl-Cl -> Br-C-Cl + H-Cl

**Express your answer in kilojoules to three significant figures.**

ΔH = -202.3 kJ

(Correct answer not provided)

### Graph Explanation

**Part B:**

Reactants: ethane (![C_2H_2](https://www.example.com/C_2H_2))

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