calculated below. H-F Bond Energy: 567 kJ/mol example H2 (g) + F2 (g) 2HF AHxn = [energy used for breaking bonds] - [energy formed in making bonds] [436 kJ/mol + 155 kJ/mol] - [2(567 kJ/mol)] = - 543 kJ/mol Average Bond Energies (kJ/mol) 436 kJ/mol 431 kJ/mol H-H С-Н 413 kJ/mol C=C 614 kJ/mol H-CI С-С 348 kJ/mol C=C 839 kJ/mol H-F 567 kJ/mol С-N 293 kJ/mol C=0 799 kJ/mol N-H 391 kJ/mol C-O 358 kJ/mol O=0 495 kJ/mol 201 kJ/mol 463 kJ/mol 146 kJ/mol N-O С-F 485 kJ/mol C=O 1072 kJ/mol O-H C-CI 328 kJ/mol C=N 615 kJ/mol O-0 C-S 259 kJ/mol N=N 418 kJ/mol F-F 155 kJ/mol Cl-CI 242 kJ/mol N=N 941 kJ/mol C=N 891 kJ/mol Estimate the enthalpy change (AHxn) of the following reactions using the bond energies above. II 1. H-H + CI-CI → H-CI + H-CI 4. H-C-CI + O C-CI H-CI CI CI нн H. H 2. O=0 Н-о-н + F-F н-с-с-н 5. H-C-H + → 0=C= + O=0 H-O-H F F H H H 3. Н-с-о-н + Н-с-о-н н-с-о-с-н + H-O-H H H H

Answered: Image /qna-images/answer/1f06f563-8dea-460f-92f0-fb8b87ad906a.jpg

Answered: calculated below. H-F Bond Energy: 567 kJ/mol example H2 (g) + F2 (g) 2HF AHxn = [energy used for breaking bonds] - [energy formed in making bonds] [436 kJ/mol…

Chemistry

10th Edition

ISBN: 9781305957404

Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher: Cengage Learning

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Question

Can you explain these questions to me please? thank you

Bond energy is defined as the amount of energy required to break a bond. These values
are positive, indicating that bond breaking is endothermic. Bond energies are reported in
kilojoules per mole (kJ/mol). The energy for breaking a hydrogen-hydrogen bond is 436
kJ/mol so when a hydrogen-hydrogen bond is formed the process releases 436 kJ/mol.
In a chemical reaction several bonds are broken and formed. For example in the
reaction below a hydrogen-hydrogen bond is broken and a fluorine-fluorine bond is broken.
Two hydrogen-fluorine bonds are formed. The overall energy change for this process is
calculated below.
H-H
Bond energy: 436 kJ/mol
F-F
Bond Energy: 155 kJ/mol
H-F
Bond Energy: 567 kJ/mol
example
H2 (g) + F2 (g)
2HF
AHX0 = [energy used for breaking bonds]- [energy formed in making bonds]
[436 kJ/mol + 155 kJ/mol] - [2(567 kJ/mol)]
=- 543 kJ/mol
Average Bond Energies (kJ/mol)
H-H
436 kJ/mol
С-Н
413 kJ/mol
C=C
614 kJ/mol
H-Cl
431 kJ/mol
C-C
348 kJ/mol
C=C
839 kJ/mol
H-F
567 kJ/mol
С-N
293 kJ/mol
C=0
799 kJ/mol
N-H
391 kJ/mol
C-O
358 kJ/mol
O=0
495 kJ/mol
N-O
201 kJ/mol
С-F
485 kJ/mol
C=0
1072 kJ/mol
O-H
463 kJ/mol
C-Cl
328 kJ/mol
C=N
615 kJ/mol
O-0
146 kJ/mol
C-S
259 kJ/mol
N=N
418 kJ/mol
F-F
155 kJ/mol
Cl-Cl
242 kJ/mol
N=N
941 kJ/mol
C=N
891 kJ/mol
Estimate the enthalpy change (AHxn) of the following reactions using the bond energies above.
II
1.
H-H + CI-CI →
H-CI + H-CI
4.
+ O
C-CI
H-CI
H-C-CI
CI
CI
нн
2. o-
H
O=0
H-O-H
+ F-F -→
н-с-с-н
5.
H-C-H +
O=C=O
H
O=0
H-O-H
F F
H.
H.
H.
3. Н-С-о-н + H-с-о-н — н-с-о-с-н
+ H-O-H
H
H
H
H
O=0-0

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