1) Given reaction O3 + NO ------------> NO2 + O2
O3 contains O=O and O-O
NO contains N=O
NO2 contains N=O and N-O
O2 contains O=O.
Then,
ΔH = Sum of bond energy of reactants - Sum of bond energy of products
= bond energy of O3 + bond energy NO - {bond energy of NO2 + bond energy of O2 }
= bond energy of (O=O + O-O) + bond energy of N=O - {bond energy of (N=O + N-O) + bond energy of O=O }
= 498 kJ/mol + 142 kJ/mol + 590 kJ/mol - {590 kJ/mol + 222 kJ/mol + 498 kJ/mol}
= -80 kJ/mol
ΔH = -80 kJ/mol
2) Given reaction H2O --------> H + OH ΔHo = 502 kJ
This is not H-H bond energy.
This is H-OH bond enthalpy.
Please help. Also, I really don't get this part. Why bond therapy of H is 502kJ...
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