Question

The reaction below forms the molecule CHFClBr starting from atoms of the elements. C + H...

The reaction below forms the molecule CHFClBr starting from atoms of the elements. C + H + F + Cl + Br → CHFClBr Given the change of energy of this reaction is ∆E= -1502 kJ and the average bond energies (in kJ/mol) C—H (413), C—Br (276), and C—Cl (328), what is the calculated value for the the C—F bond energy? Blank 1 kJ/mol Hint: (1) This question asks you to think about solving "backwards" from the way most of the other questions in this PiQ are phrased.

Delta E(rxn) = 0 -  [H(C-H) + H(C-Cl) + H(C-F) + H(C-Br)]

-1502 = -(413 + 328 + x + 276)

1502 = 1017 + x

x = 485 KJ/mol .... Answer

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