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Question

Print n 10 of 12 (1 point) Incorrect Incorrect Incorrect xI ct × Incorrect Incorrect Use the bond dissociation energies of the following table to estimate the molar change in free energy of the reaction of H2C-CH2 and H-Br to yield H3C-CH2Br: Some Homolytic Bond Dissociation Energies I-I Br-Br 46.1 kcal/mol H3C-CH3 90.1 Cl-Cl | 59.0 kcal/mol | H2C=CH2 | 66.0 F-F 38.0 kcal/mol H2C-CH2 174.1 H-H 104.2 kcal/mol I-CH3 H-1 71.3 kcal/mol Br- CH3 72.1 H-Br 87.5 kcal/mol Cl-CH3 83.7 H-CI 103.2 kcal/mol F-CH3 H-F 136.3 kcal/mol Number 36.1 kcal/mol H-CH2CH3 101.1 10.5 kcal/ mol kcal/mol kcallmolThe H2C-CH2 bond is broken in this reaction, which costs 66.0 kcal/mol of r bond) kcal/molenergy. What other bond is broken? What two bonds are formed? What is the difference in the total energies of the kcal/mol bonds formed and the bonds broken? 57.6 kcal/mol kcal/mol kcal/mol 115.0 kcal/mol

Explanation / Answer

ANSWER:

The balanced chemical equation is:

CH2=CH2 + HBr ---------> CH3-CH2Br

Energy change of the reaction = Bond dissociation energy of broken bonds - Bond dissociation energy new formed bonds

Energy change of the reaction = [ D C=c + DHBr] - [ DC-H + DC-Br]

D = bond dissociation energy and subscript shows the type of bond, e.g D C=c means bond dissociation enegy of pi bond.

Energy change of the reaction = [ 66.0 KCal/mol + 87.5KCal/mol] - [101.1KCal/mol + 72.1KCal/mol]

Energy change of the reaction = 153.5KCal/mol - 173.2 KCal/mol = - 19.7KCal/mol

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