Use the table of Bond Energies (BE) in the table below to calculate the Heat of Reaction, AHxg for the complete combustion of two moles of liquid ethanal (CH3CHO (1): 2 CH3CHO (1) + 5 02(9) + 4 CO2 (9) + kJ H-C-C 0 =0 O =C=0 Н-О-Н TABLE 9.5 Bond Energies (in kJ/mol)* Single Bonds H N F Br H 432 411 346 386 305 167 459 358 201 142 S 363 272 226 F 565 485 283 190 284 155 CI 428 327 313 218 255 249 240 Br 362 285 201 217 249 216 190 295 213 201 278 208 175 149 Multiple Bonds C=C 602 C=N 615 C=0 745 (799 in CO,) C=C 835 C=N 887 C=0 1072
Use the table of Bond Energies (BE) in the table below to calculate the Heat of Reaction, AHxg for the complete combustion of two moles of liquid ethanal (CH3CHO (1): 2 CH3CHO (1) + 5 02(9) + 4 CO2 (9) + kJ H-C-C 0 =0 O =C=0 Н-О-Н TABLE 9.5 Bond Energies (in kJ/mol)* Single Bonds H N F Br H 432 411 346 386 305 167 459 358 201 142 S 363 272 226 F 565 485 283 190 284 155 CI 428 327 313 218 255 249 240 Br 362 285 201 217 249 216 190 295 213 201 278 208 175 149 Multiple Bonds C=C 602 C=N 615 C=0 745 (799 in CO,) C=C 835 C=N 887 C=0 1072
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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Hi! Could I get this answered confirmed. I recieved a good answer, but want to make sure it's right and to see if there is any other way to do it. Possible answers are -1060, -2120, -2090, and +1920. Thanks!
![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%2F05ba1ec5-93ed-499f-a27b-b6751d02142d%2Fr8esbkk_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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