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To determine the enthalpy change for the reaction using bond energies, we use the formula:

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To determine the enthalpy change for the reaction using bond energies, we use the formula:

ΔHreaction∘=∑(Bond energies of bonds broken)−∑(Bond energies of bonds formed)\Delta H^\circ_{reaction} = \sum (\text{Bond energies of bonds broken}) - \sum (\text{Bond energies of bonds formed})

The reaction is:
CH₃COCH₃ + NH₂OH → (CH₃)₂C=NOH + H₂O

First, let's identify all the bonds in the reactants and products.

Reactants:

  1. CH₃COCH₃ (Propanone)

    • 6 C-H bonds
    • 2 C-C bonds
    • 1 C=O bond

  2. NH₂OH (Hydroxylamine)

    • 2 N-H bonds
    • 1 N-O bond
    • 1 O-H bond

    Total bonds in reactants:

    • 6 C-H
    • 2 C-C
    • 1 C=O
    • 2 N-H
    • 1 N-O
    • 1 O-H

    Products:

  3. (CH₃)₂C=NOH (Propanone oxime)

    • 6 C-H bonds
    • 2 C-C bonds
    • 1 C=N bond
    • 1 N-O bond
    • 1 O-H bond

  4. H₂O (Water)

    • 2 O-H bonds

    Total bonds in products:

    • 6 C-H
    • 2 C-C
    • 1 C=N
    • 1 N-
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