Ammonia is produced directly from nitrogen and hydrogen by using the Haber process. The chemical reaction is
Question:
N2 (g) + 3H2 (g) 2NH3 (g)
(a) Use Table 8.4 to estimate the enthalpy change for the reaction. Is it exothermic or endothermic?
(b) Compare the enthalpy change you calculate in (a) to the true enthalpy change as obtained using ÎHof values.
Transcribed Image Text:
TABLE 8.4 Single Bonds e Average Bond Enthalpies (kJ/mol) C H C-C C-N с_o C-F C CI C Br 413 348 293 358 485 328 276 240 259 N H N-N 391 163 201 272 200 243 463 146 190 203 234 F-F 155 O-O CI-F CI-CI 253 242 O Cl N F N-CI N Br 237 218 193 S--H BrCl 436 SF 567 431 366 299 339 327 253 218 266 S-CI SBr CS H-Cl H Br I- Cl I Br 208 175 151 Si-H SiSi SiC Si-O SiCl 323 226 301 368 464 Multiple Bonds с-с 614 839 615 891 799 1072 418 O 941 607 S O 495 C-N N-O 523 418 S-S
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Related Book For
Chemistry The Central Science
ISBN: 978-0321696724
12th edition
Authors: Theodore Brown, Eugene LeMay, Bruce Bursten, Catherine Murphy, Patrick Woodward
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