Given that Δ H ∘ f [ H ( g ) ] = 218.0 kJ ⋅ mol − 1 Δ H ∘ f [ C ( g ) ] = 716.7 kJ ⋅ mol − 1 Δ H ∘ f [ CH 4 ( g ) ] = − 74.6 kJ ⋅ mol − 1 calculate the average molar bond enthalpy of the carbon‑hydrogen bond in a CH 4 molecule

Average molar bond enthalpy of C-H bond in is 415.825 kJ/mol.

Explanation:

Reaction:

Heat of reaction (energy needed to break 4 moles of C-H bond in 1 mol of ) =

        =

1 mol of contain 4 moles of C-H bonds.

So, average molar bond enthalpy of C-H bond in

     =

     = 415.825 kJ/mol

the answer would be a

i would say b

explanation:

but i think i would need more information than that