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For the reaction below: H CI. H-CI a. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the OWL Table Reference, not data from your text. Click the References button and then click the Tables link on the drop-down that appears. Include algebraic sign and units. b. Is the reaction exothermic or endothermic? O c. Is the reaction likely to proceed spontaneously in the direction written? Ⓒ

For the reaction below: H CI. H-CI a. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the OWL Table Reference, not data from your text. Click the References button and then click the Tables link on the drop-down that appears. Include algebraic sign and units. b. Is the reaction exothermic or endothermic? O c. Is the reaction likely to proceed spontaneously in the direction written? Ⓒ

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter7: Chemical Energy
Section: Chapter Questions
Problem 16Q: For the reaction HgO(s)Hg(l)+12O2(g),H=+90.7KJ: a. What quantity of heat is required to produce 1...
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Bond Dissociation Energies Bond Dissociation Energies, Dº298, for X-Y kJ/mol (kcal/mol) H F X\Y= CI Br I OH NH₂ CN CH3- 439 (105) 452 (108) 356 (85) 293 (70) 238 (57) 385 (92) 356 (85) 510 (122) CH3CH₂- 423 (101) 444 (106) 335 (80) 285 (68) 228 (53) 380 (91) 356 (85) 336 (80) (CH3)2CH- 409 (98) 448 (107) 339 (81) 274 (65) 226 (54) 385 (92) (CH3)3C- 404 (97) 331 (79) 263 (63) 213 (51) 380 (91) CH₂=CHCH2- 362 (86.5) 289 (69) 230 (55) 172 (41) CH₂ 376 (90) 301 (72) 243 (58) 201 (48) CH₂=CH- 465 (111) 368 (87) 259 (62) 536 (128) 473 (113) 527 (126) 402 (96) 337 (80.5) 274 (65) 464 (111) 427 (102) 377 (90) CH30- 436 (104) 333 (80) H- 435 (104) 569 (136) 431 (103) 368 (88) 297 (71) 498 (119) 449 (107) 439 (105) 423 (101) 543 (130) Most data from CRC handbook of Chemistry and Physics, 85th ed., D. R. Lide, ed., CRC press, Boca Raton, FL, 2004, p 9-65. Uncertainties range from less than 1 kJ/mol to ca. 20 kJ/mol (5 kcal/mol) and are listed in the CRC handbook CH3 377 (90) 368 (88) 351(84) 339 (81) 305 (73) 332 (79) 406 (97) CH3CH2- 368 (88)
Transcribed Image Text:Bond Dissociation Energies Bond Dissociation Energies, Dº298, for X-Y kJ/mol (kcal/mol) H F X\Y= CI Br I OH NH₂ CN CH3- 439 (105) 452 (108) 356 (85) 293 (70) 238 (57) 385 (92) 356 (85) 510 (122) CH3CH₂- 423 (101) 444 (106) 335 (80) 285 (68) 228 (53) 380 (91) 356 (85) 336 (80) (CH3)2CH- 409 (98) 448 (107) 339 (81) 274 (65) 226 (54) 385 (92) (CH3)3C- 404 (97) 331 (79) 263 (63) 213 (51) 380 (91) CH₂=CHCH2- 362 (86.5) 289 (69) 230 (55) 172 (41) CH₂ 376 (90) 301 (72) 243 (58) 201 (48) CH₂=CH- 465 (111) 368 (87) 259 (62) 536 (128) 473 (113) 527 (126) 402 (96) 337 (80.5) 274 (65) 464 (111) 427 (102) 377 (90) CH30- 436 (104) 333 (80) H- 435 (104) 569 (136) 431 (103) 368 (88) 297 (71) 498 (119) 449 (107) 439 (105) 423 (101) 543 (130) Most data from CRC handbook of Chemistry and Physics, 85th ed., D. R. Lide, ed., CRC press, Boca Raton, FL, 2004, p 9-65. Uncertainties range from less than 1 kJ/mol to ca. 20 kJ/mol (5 kcal/mol) and are listed in the CRC handbook CH3 377 (90) 368 (88) 351(84) 339 (81) 305 (73) 332 (79) 406 (97) CH3CH2- 368 (88)
For the reaction below: H O". CI. H-CI a. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the OWL Table Reference, not data from your text. Click the References button and then click the Tables link on the drop-down that appears. Include algebraic sign and units. b. Is the reaction exothermic or endothermic? Ⓒ c. Is the reaction likely to proceed spontaneously in the direction written?
Transcribed Image Text:For the reaction below: H O". CI. H-CI a. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the OWL Table Reference, not data from your text. Click the References button and then click the Tables link on the drop-down that appears. Include algebraic sign and units. b. Is the reaction exothermic or endothermic? Ⓒ c. Is the reaction likely to proceed spontaneously in the direction written?
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