Bond dissociation energy (BDE) is defined as energy needed to breakup a specific

Question

Bond dissociation energy (BDE) is defined as energy needed to breakup a specific
bond in a molecule. We can also consider it to be an enthalpy ofthe bond breaking
reaction. Using this reasoning and BDE of molecular oxygen (O2)estimate the
enthalpy of formation of O radical (Hf O). BDE of O2 is 495 kJ/mol.Write a
balanced chemical equation first and show schematically allenthalpies of formation
and an enthalpy of reaction. You can figure out the rightanswer from that scheme.

Please be detailed and will rate for sure

Explanation / Answer

O2 = >    2 O* delH_rxn = H_broken - H_formed = 495 - 0 = 495kJ/mol        (note O=O bondbroken homolytically; no bonds formed) Formation of 1 mol O* radical 0.5*O2 => O* delH_formation = 0.5*delH_rxn = 0.4*495 = 247.5 kJ/mol ~248kJ/mol

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