From the following bond energies
`H-H` bond energy `431.37 kJ mol^(-1)`
`C=C` bond energy `606.10 kJ mol^(-1)`
`C-C` bond energy `336.49 kJ mol^(-1)`
`C-H` bond energy `410.5 kJ mol^(-1)`
Enthalpy for the reaction
`overset(H)overset(|)underset(H)underset(|)(C )=overset(H)overset(|)underset(H)underset(|)(C )+H-HtoH-overset(H)overset(|)underset(H)underset(|)(C )-overset(H)overset(|)underset(H)underset(|)(C )-H`
will be

Options

A. 553.0kJ `mol^(-1)`
B. 1523.6 kJ `mol^(-1) `
C. `-243.6 " kJ mol"^(-1)`
D. `-120.0 "kJ mol"^(-1)`

Answer

D

Explanation

`DeltaH` = dissociation energy of reactant -Bond dissociation of energy of product .
`DeltaH=(606.10+4xx410.5+431.37)-(6xx410.50+336.49)`
` =-120.0 kJ//"mol"`