Use the tables below to determine the enthalpy of reaction (in kJ) for the following balanced chemical equation: Table T16-5-1. BDES, average single bond dissociation energies (in kJ/mol) I Br CI s P si F ONC H 299 366 431 368 322 323 568 463 391 413 436 220 276 328 259 264 301 453 358 276 348 N 159 243 200 200 335 272 176 193 234 234 203 364 340 368 190 146 F 277 237 193 327 490 582 157 Si 234 310 464 226 226 184 264 319 209 218 253 266 CI 208 218 242 Br 175 193 I 151 Multiple Bonds (BDE in kJ/mol) Bond BDE Bond BDE N=N 418 C=C 620 NEN 941 C=C 815 C=N 615 C=0 745 CEN 891 C=O 1072 N=O 607 O=0 499 Reaction: C2H4 + l2 -> C2H412 P.

Use the tables below to determine the enthalpy of reaction (in kJ) for the following balanced chemical equation: Table T16-5-1. BDES, average single bond dissociation energies (in kJ/mol) I Br CI s P si F ONC H 299 366 431 368 322 323 568 463 391 413 436 220 276 328 259 264 301 453 358 276 348 N 159 243 200 200 335 272 176 193 234 234 203 364 340 368 190 146 F 277 237 193 327 490 582 157 Si 234 310 464 226 226 184 264 319 209 218 253 266 CI 208 218 242 Br 175 193 I 151 Multiple Bonds (BDE in kJ/mol) Bond BDE Bond BDE N=N 418 C=C 620 NEN 941 C=C 815 C=N 615 C=0 745 CEN 891 C=O 1072 N=O 607 O=0 499 Reaction: C2H4 + l2 -> C2H412 P.

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 52E: Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00...

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