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Problem 5.84 Use bond enthalpies in the table below to estimate ΔH for each of the...

Problem 5.84

Use bond enthalpies in the table below to estimate ΔH for each of the following reactions

.
Average Bond Enthalpies (kJ/mol)
C−H413 N−H391 O−H463 F−F155
C−C348 N−N163 O−O146
C=C614 N−O201 O=O495 Cl−F253
C−N293 N−F272 O−F190 Cl−Cl242
C−O358 N−Cl200 O−Cl203 Br−F237
C=O799 N−Br243 O−I234 Br−Cl218
C−F485 H−H436 Br−Br193
C−Cl328 H−F567
C−Br276 H−Cl431 I−Cl208
C−I240 H−Br366 I−Br175
H−I299 I−I151

Part A

Br-C H+ CI CI

Express your answer in kilojoules to 3 significant figures.

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Part B

5.84b.jpg

Express your answer in kilojoules to 3 significant figures.
kJ
Br-C H+ CI CI
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Answer #1

Part A The chemical reaction is written as follows: BrCCICI_H Bond enthalpy of C-H-413 kJ/mol Bond enthalpy of C-Br276 kJ/mol Bond enthalpy of Cl-Cl-242 kJ/mol Bond enthalpy of C-Cl-328 kJ/mol Bond enthalpy of Cl-H 431 kJ/mol The enthalpy of reaction is expressed as follows: AH - Bond enthalpy(reactant) - > Bond enthalpy(product) The enthalpy of reaction is calculated as follows: CH + BCI-cl--(3 × B CI-H ci-cl C-CI 413 kJ/mol242 kJ/mol - 328 kJ/mol - 431 kJ/mol 1-104 kJ/mol

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Answer #2
Use the bond enthalpies in the table below to calculate a numerical estimate of delta h for the reaction
source: AP Chemistry
answered by: Smith
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