The standard enthalpy of formation ( $∆$ H_f⁰ ) at 298 K for methane,CH_4(g), is 74.8 KJ/mol. The additional information required to determine the average energy for C-H bond formation would be

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The dissociation energy of hydrogen molecule, H₂

Latent heat of vaporisation of methane.

The first four ionisation energies of carbon and electron gain enthalpy of hydrogen

The dissociation energy of H₂ and enthalpy of sublimation of carbon

answer is B.

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Detailed Solution

Heat of formation of CH₄ is represented as

C_(g) + 2H_2(g) $\to$ CH_4(g)

standard condition of carbon is graphite and is converted into gaseous carbon, sublimation energy is required

H₂ molecule is dissociated into hydrogen atoms, bond dissociation energy of hydrogen molecule is required

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