JEE Mains · Chemistry · STD 11 - 5. Thermodynamics and thermochemistry
The standard enthalpy of formation \((\Delta _f\,H^o_{298})\) for methane, \(CH_4\) is \(-74.9\,kJ\,mol^{-1}\) . In order to calculate the average energy given out in the formation of a \(C - H\) bond from this it is necessary to know which one of the following?
- A The dissociation energy of the hydrogen molecule, \(H_2\)
- B The first four ionisation energies of carbon.
- C The dissociation energy of \(H_2\) and enthalpy and sublimation of carbon (graphite).
- D The first four ionisation energies of carbon and electron affinity of hydrogen.
Answer & Solution
Correct Answer
(A) The dissociation energy of the hydrogen molecule, \(H_2\)
Step-by-step Solution
Detailed explanation
To calculate average enthalpy of \(C-H\) bond in methane following informations are needed \((i)\) dissociation energy of \(H_2\) i.e. \(\frac{1}{2}{H_2}(g) \to H(g);\Delta H = x\) (suppose) \((ii)\) Sublimation enegry of \(C\) (graphite) to \(C(g)\)…
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