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 =kJHH-C-C0 =0 0=C=0Н-О-НHH.TABLE 9.5Bond Energies (in kJ/mol)*Single BondsHNFCIBrH432C411346386305167459358201142S363272226--F565485283190284155CI218255428327313249240Br362285201217249216190I295213201278208175149-Multiple BondsC=C602C=N615C=0745 (799 in CO,)C=C835C=N887C=01072N=N418N=O607S=0 (in SO,)532NEN9420=0494S=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 =| Selectv 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/moleH20(g)= - 241.8 kJ/mole

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• 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

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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