Average Bond Energies (kJ/mol) Single Bonds Multiple Bonds H-H H-F H-CI 432 N-H 391 149 C=C 614 565 N-N 160 208 C=C 839 427 N-F 272 -Br 175 0=0 495 N-CI H-Br H–I 363 295 200 243 C=0* 745 N-Br S-H 347 C=0 1072 N-O 201 S-F 327 N=0 607 C-H 413 0-H 467 S-CI 253 N=N 418 C-C 347 0-0 146 S-Br 218 N=N 941 C-N 305 O-F 190 S-S 266 C=N 615 C-O C-F 0-CI 0-I 358 203 CEN 891 485 234 Si-Si 340 C-CI 339 Si-H 393 С—Br 276 F-F 154 Si-C 360 C–I 240 F-CI 253 Si-O 452 F-Br C-CI C-S 259 237 239 C-Br 218 Br-Br 193 *C=0 (CO2) = 799

Average Bond Energies (kJ/mol) Single Bonds Multiple Bonds H-H H-F H-CI 432 N-H 391 149 C=C 614 565 N-N 160 208 C=C 839 427 N-F 272 -Br 175 0=0 495 N-CI H-Br H–I 363 295 200 243 C=0* 745 N-Br S-H 347 C=0 1072 N-O 201 S-F 327 N=0 607 C-H 413 0-H 467 S-CI 253 N=N 418 C-C 347 0-0 146 S-Br 218 N=N 941 C-N 305 O-F 190 S-S 266 C=N 615 C-O C-F 0-CI 0-I 358 203 CEN 891 485 234 Si-Si 340 C-CI 339 Si-H 393 С—Br 276 F-F 154 Si-C 360 C–I 240 F-CI 253 Si-O 452 F-Br C-CI C-S 259 237 239 C-Br 218 Br-Br 193 *C=0 (CO2) = 799

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 82QRT: The molecular structure shown is of one form of glucose, C6H12O6 Glucose can be oxidized to carbon...

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The molecular structure shown is of one form of glucose, C6H12O6 Glucose can be oxidized to carbon dioxide and water according to the equation C6H12O6(S) + 6 O2(g)6 CO2(g) + 6 H2O(g) (a) Using the method described in Section 6-6a for estimating enthalpy changes from bond energies, estimate rH for the oxidation of this form of glucose. Make a list of all bonds broken and all bonds formed in this process. (b) Compare your result with the experimental value of 2816 kJ/mol for combustion of glucose. Why might there be a difference between this value and the one you calculated in part (a)?
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