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The observed heat of formation of CH3COOH(g) is -439 kJ. The enthalpy of resonance of CH3COOH(g) is X kJ from the given data. Find the value of |X|.
Bond energy (kJ)Heat of atomization(kJ)C-H = 413C (solid)=716C-C = 348H2=436C=O = 732O2=498C-O = 351O-H = 463

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Solution

2C(s)+2H2(g)+O2CH3COOH(g)without resonance
ΔHf=(716×2)+(436×2)+498(413×3)348732351463=331 kJ
CH3COOH(without resonance)CH3COOH (with resonance)
ΔHreso=439(331)=108 kJ

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