The change in energy Δ E is to be calculated from bond energy values for the given reactions. Concept introduction: The bond energy is the energy required to break apart a compound. Energy change of a reaction is defined as the sum of change in internal energy and the product of absolute temperature and entropy of system. To determine: The value of energy change Δ E for the reaction H 2 + Cl 2 → 2 HCl .
The change in energy Δ E is to be calculated from bond energy values for the given reactions. Concept introduction: The bond energy is the energy required to break apart a compound. Energy change of a reaction is defined as the sum of change in internal energy and the product of absolute temperature and entropy of system. To determine: The value of energy change Δ E for the reaction H 2 + Cl 2 → 2 HCl .
Solution Summary: The author explains that the change in energy Delta E is to be calculated from bond energy values for the given reactions.
Interpretation: The change in energy ΔE is to be calculated from bond energy values for the given reactions.
Concept introduction: The bond energy is the energy required to break apart a compound.
Energy change of a reaction is defined as the sum of change in internal energy and the product of absolute temperature and entropy of system.
To determine: The value of energy change ΔE for the reaction H2+Cl2→2HCl.
(b)
Interpretation Introduction
Interpretation: The change in energy ΔE is to be calculated from bond energy values Interpretation: The change in energy ΔE is to be calculated from bond energy values for the given reactions.
Concept introduction: The bond energy is the energy required to break apart a compound.
Energy change of a reaction is defined as the sum of change in internal energy and the product of absolute temperature and entropy of system.
To determine: The value of energy change ΔE for the reaction N≡N+3H2→2NH3.
Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxn for the equation
NH3 (g) + 2 O2 (g) --> HNO3 (g) + H20 (g)
Average molar bond enthalpies. (?bond)
Bond
??⋅???−1
Bond
??⋅???−1
O−H
464
C≡N
890
O−O
142
N−H
390
C−O
351
N−O
201
O=O
502
N=N
418
C=O
730
N=O
607
C−C
347
F−F
155
C=C
615
Cl−Cl
243
C≡C
811
Br−Br
192
C−H
414
H−H
435
C−F
439
H−F
565
C−Cl
331
H−Cl
431
C−Br
276
H−Br
368
C−N
293
H−S
364
C=N
615
S−S
225
A.) What is the heat of reaction, ΔH°?
CO2(g) + H2O(l) à H2CO3(aq)
–20.2 kJ mol–1
–1379 kJ mol–1
–592 kJ mol–1
B.)
What is the average bond energy in CO2?
CO2(g) ΔH°f, = –393.5 kJ mol–1
CO(g) ΔH°f, = –110.5 kJ mol–1
C(g) ΔH°f, = +715 kJ mol–1
CO32–(aq) ΔH°f, = –676.3 kJ mol–1
O(g) ΔH°f, = +249.0 kJ mol–1
207 kJ mol–1
1607 kJ mol–1
804 kJ mol–1
Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxnΔHrxn° for the equation
C2H4 (g) + HBr (g) --> C2H5Br (g)
Average molar bond enthalpies. (?bond)(Hbond)
Bond
??⋅???−1kJ⋅mol−1
Bond
??⋅???−1kJ⋅mol−1
O−HO−H
464464
C≡NC≡N
890890
O−OO−O
142142
N−HN−H
390390
C−OC−O
351351
N−NN−N
159159
O=OO=O
502502
N=NN=N
418418
C=OC=O
730730
N≡NN≡N
945945
C−CC−C
347347
F−FF−F
155155
C=CC=C
615615
Cl−ClCl−Cl
243243
C≡CC≡C
811811
Br−BrBr−Br
192192
C−HC−H
414414
H−HH−H
435435
C−FC−F
439439
H−FH−F
565565
C−ClC−Cl
331331
H−ClH−Cl
431431
C−BrC−Br
276276
H−BrH−Br
368368
C−NC−N
293293
H−SH−S
364364
C=NC=N
615615
S−SS−S
225225
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Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY