Energy required to break all four C-H bonds in methane is 1662 kJ/mol. Calculate the average bond enthalpy for methane molecule.

436 kJ/mol

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332 kJ/mol

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208 kJ/mol

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416 kJ/mol

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Solution

The correct option is D
416 kJ/mol

In polyatomic molecules the term mean or average bond enthalpy is used.

It is calculated by dividing the total bond dissociation enthalpy by number of bonds broken.

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Similar questions

H_{2} (g)

436 kJ/mol

N_{2} (g)

941.3 kJ/mol

Δ H_{f}^{\circ} (N H_{3}) = - 46 kJ/mol

Use bond energies to estimate the enthalpy of formation of HBr(g).
BE(H-H) = 436 kJ/mol
BE(Br-Br) = 192 kJ/mol
BE(H-Br) = 366 kJ/mol

C H_{4} (g)

360 k c a l m o l^{- 1}

C - - H

k c a l m o l^{- 1}

F_{2}

X e F_{4} \to X e^{+} + F^{-} + F_{2} + F

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