From the following bond energies : H − H bond energy : 431.37 kJ mol − 1 C = C bond energy : 606.10 kJ mol − 1 C − C bond energy : 336.49 kJ mol − 1 C − H bond energy : 410.50 kJ mol − 1 Enthalpy for

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From the following bond energies : H − H bond energy : 431.37 kJ mol − 1 C = C bond energy : 606.10 kJ mol − 1 C − C bond energy : 336.49 kJ mol − 1 C − H bond energy : 410.50 kJ mol − 1 Enthalpy for the reaction, will be :NEET 2009 (Mains)

TestHub · Accepted Answer

Δ H = dissociation energy of reactant - Bond dissociation of energy of product. Δ H = ​ ( 606.10 + 4 × 410.5 + 431.37 ) − ( 6 × 410.50 + 336.49 ) = − 120.0 kJ / mol ​

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