Hydrogenation reactions are used to add hydrogen across double bonds in hydrocarbons and other organic compounds. use average bond energies to calculate δhrxn for the hydrogenation reaction.

H2 (g) + C2H4 (g) →C2H6 (g)

H-H + H2C = CH2→H3C-Ch3

2C - H bonds and one C-C bond are formed while enthalpy change (dH) of the reaction,

H-H: 432kJ/mol

C=C: 614kJ/mol

C-C: 413 kJ/mol

C-C: 347 kJ/mol

dH is equal to sum of the energies released during the formation of new bonds or negative sign, and sum of energies required to break old bonds or positive sign.

The bond which breaks energy is positive.

432+614 = 1046kJ/mol

Formation of bond energy is negative

2 (413) + 347 = 1173 kJ/mol

dH reaction is - 1173 + 1046 = - 127kJ/mol