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QJEEM06Che351: JEE Main 2006 Chemistry - Class 11 JEEM06Che351 Solution: The standard enthalpy of formation Δ f H o at 298 K for…

The standard enthalpy of formation ΔfHo at 298 K for methane, CH4(g), is –74.8 kJ mol–1. The additional information required to determine the average energy for C – H bond formation would be :

Multiple Choice Options

  • A the dissociation energy of H2 and enthalpy of sublimation of carbon
  • B latent heat of vapourization of methane
  • C the first four ionization energies of carbon and electron gain enthalpy of hydrogen
  • D the dissociation energy of hydrogen molecule, H2

Step-by-Step Verified Solution

The standard enthalpy of formation of CH4 is given by the equation :

C(s)+2H2(g)→CH4(g)

In order to calculate average energy for C – H bond formation we should know the following data.

C(graphite) → C(g) ; ΔHfo = enthalpy of sublimation of carbon

H2(g) → 2H(g) ; ΔH = bond dissociation energy of H2

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