• Use the table of Bond Energies (BE) in the table below to calculate the Heat of Reaction, AHxn for the complete combustion of two moles of liquid ethanal (CH3CHO (1): 2 CH3CHO () + 5 02(9) → 4 CO2 (g) + 4 H20(9) AHrxn kJ H 0 =0 0=C=0 H-C-C H. H-O-H TABLE 9.5 Bond Energies (in kJ/mol)* Single Bonds H N F CI Br H 432 C 411 346 386 305 167 459 358 201 142 S 363 272 226 F 565 485 283 190 284 155 CI 428 327 313 218 255 249 240 Br 362 285 201 217 249 216 190 I 295 213 201 278 208 175 149 Multiple Bonds C=C 602 C=N 615 c=0 745 (799 in CO,) C=C 835 C=N 887 C=0 1072 N=N 418 N=O 607 S=0 (in SO,) 532 N=N 942 0=0 494 S=0 (in SO,) 469 *Data are taken from J. E. Huheey, Keiter, and Keiter, Inorganic Chemistry, 4th ed. (New York: HarperCollins, 1993), pp. A21-A34. AHxa = ( Select ) v kJ / (2 mol CH3CHO (1) ) Use the: • Heat of Reaction AHrxn values for the combustion of two moles of liquid ethanal (CH3CHO () • the Enthalpies of Formation (AH;º) for carbon dioxide (CO2(9)) and water (H20(9) to calculate the: • Enthalpy of Formation (AHF° ) of 1 mole of liquid ethanal (CH3CHO (1) ): AH;° = ISelect] v kJ/mol CH3CHO (1) Enthalpies of Formation: CO2(g) AHf° = - 393.5 kJ/mole H20(g) AH:° = - 241.8 kJ/mole
• Use the table of Bond Energies (BE) in the table below to calculate the Heat of Reaction, AHxn for the complete combustion of two moles of liquid ethanal (CH3CHO (1): 2 CH3CHO () + 5 02(9) → 4 CO2 (g) + 4 H20(9) AHrxn kJ H 0 =0 0=C=0 H-C-C H. H-O-H TABLE 9.5 Bond Energies (in kJ/mol)* Single Bonds H N F CI Br H 432 C 411 346 386 305 167 459 358 201 142 S 363 272 226 F 565 485 283 190 284 155 CI 428 327 313 218 255 249 240 Br 362 285 201 217 249 216 190 I 295 213 201 278 208 175 149 Multiple Bonds C=C 602 C=N 615 c=0 745 (799 in CO,) C=C 835 C=N 887 C=0 1072 N=N 418 N=O 607 S=0 (in SO,) 532 N=N 942 0=0 494 S=0 (in SO,) 469 *Data are taken from J. E. Huheey, Keiter, and Keiter, Inorganic Chemistry, 4th ed. (New York: HarperCollins, 1993), pp. A21-A34. AHxa = ( Select ) v kJ / (2 mol CH3CHO (1) ) Use the: • Heat of Reaction AHrxn values for the combustion of two moles of liquid ethanal (CH3CHO () • the Enthalpies of Formation (AH;º) for carbon dioxide (CO2(9)) and water (H20(9) to calculate the: • Enthalpy of Formation (AHF° ) of 1 mole of liquid ethanal (CH3CHO (1) ): AH;° = ISelect] v kJ/mol CH3CHO (1) Enthalpies of Formation: CO2(g) AHf° = - 393.5 kJ/mole H20(g) AH:° = - 241.8 kJ/mole
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.86QE: One of the components of jet engine fuel is n-dodecane, C12H26(), which has a standard enthalpy of...
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![Use the table of Bond Energies (BE) in the table below to calculate the Heat of Reaction, AHrxn for the complete combustion of two moles of liquid ethanal (CH3CHO (1):
2 CH3CHO (1) + 5 02(9) 4 CO2 (g)
+ 4 H20(9) AHrxn =
kJ
H
H-C-C
0 =0 0=C=0
Н-О-Н
H
H.
TABLE 9.5
Bond Energies (in kJ/mol)*
Single Bonds
H
N
F
CI
Br
H
432
C
411
346
386
305
167
459
358
201
142
S
363
272
226
-
-
F
565
485
283
190
284
155
CI
218
255
428
327
313
249
240
Br
362
285
201
217
249
216
190
I
295
213
201
278
208
175
149
-
Multiple Bonds
C=C
602
C=N
615
C=0
745 (799 in CO,)
C=C
835
C=N
887
C=0
1072
N=N
418
N=O
607
S=0 (in SO,)
532
NEN
942
0=0
494
S=0 (in SO,)
469
*Data are taken from J. E. Huheey, Keiter, and Keiter, Inorganic Chemistry, 4th ed. (New York:
НaгрerCollins, 1993), рр. А21-А34.
AHPXD =
| Select
v kJ / (2 mol CH3CHO (1) )
Use the:
• Heat of Reaction AHrxn values for the combustion of two moles of liquid ethanal (CH3CHO ()
• the Enthalpies of Formation (AH;°) for carbon dioxide (CO2(9) and water (H20()
to calculate the:
• Enthalpy of Formation (AHF° ) of 1 mole of liquid ethanal (CH3CHO () ):
AH;° = ( Select]
v kJ/mol CH3CHO (1)
Enthalpies of Formation:
CO2(g)
AH;° = - 393.5 kJ/mole
H20(g)
= - 241.8 kJ/mole](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F66173c1a-f883-4b2a-9c4a-34112153fb2f%2Fdccf68bd-4d14-4c40-a085-b868614dd538%2F49v8he_processed.png&w=3840&q=75)
Transcribed Image Text:Use the table of Bond Energies (BE) in the table below to calculate the Heat of Reaction, AHrxn for the complete combustion of two moles of liquid ethanal (CH3CHO (1):
2 CH3CHO (1) + 5 02(9) 4 CO2 (g)
+ 4 H20(9) AHrxn =
kJ
H
H-C-C
0 =0 0=C=0
Н-О-Н
H
H.
TABLE 9.5
Bond Energies (in kJ/mol)*
Single Bonds
H
N
F
CI
Br
H
432
C
411
346
386
305
167
459
358
201
142
S
363
272
226
-
-
F
565
485
283
190
284
155
CI
218
255
428
327
313
249
240
Br
362
285
201
217
249
216
190
I
295
213
201
278
208
175
149
-
Multiple Bonds
C=C
602
C=N
615
C=0
745 (799 in CO,)
C=C
835
C=N
887
C=0
1072
N=N
418
N=O
607
S=0 (in SO,)
532
NEN
942
0=0
494
S=0 (in SO,)
469
*Data are taken from J. E. Huheey, Keiter, and Keiter, Inorganic Chemistry, 4th ed. (New York:
НaгрerCollins, 1993), рр. А21-А34.
AHPXD =
| Select
v kJ / (2 mol CH3CHO (1) )
Use the:
• Heat of Reaction AHrxn values for the combustion of two moles of liquid ethanal (CH3CHO ()
• the Enthalpies of Formation (AH;°) for carbon dioxide (CO2(9) and water (H20()
to calculate the:
• Enthalpy of Formation (AHF° ) of 1 mole of liquid ethanal (CH3CHO () ):
AH;° = ( Select]
v kJ/mol CH3CHO (1)
Enthalpies of Formation:
CO2(g)
AH;° = - 393.5 kJ/mole
H20(g)
= - 241.8 kJ/mole
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