The enthalpy of formation of H2\(_{o}\) (l) is - 285.77 kJ mol\(^{-1}\). The enthalpy of neutralisation of a strong acid and a strong base is - 56.07 kJ mol\(^{-1}\). What is the enthalpy of formation of OH\(^{-}\)ion? Please help me get the correct answer and explain it.
- 229.70 kJ
+ 229.70 kJ
+ 350.75 kJ
- 350.75 kJ
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Click Here to Post AnswerH2I+2BOH⇒2BI+2H2O=ΔH=−285.77kJ/mol
H+OH–⇒H2O;ΔH==−56.07kJ/mol
The heat of ionization or the energy of dissociation in this reaction is equal to (–285.77 + 56.07) kJ/mol =-229.7 KJ/mol
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