If resonance energy of benzene is -150.4kJ/mol. Bond dissociation enthalpy of H2, Cl2 and HCl are 434, 242 and 431 kJ mol ^-1 respectively. it says: use the enthalpy of hydrogenation data to calculate a value for the enthalpy of hydrogenation of cyclohex 1, 4 diene then it says predict the value of the enthalpy of hydrogenation for cyclohex 1,3 diene thanks il definitely check that out! If resonance energy of benzene is -150.4 kJ mol-1, its enthalpy of hydrogenation would be, The correct option is : (c) - 208.1 kJ mol-1, = 3 x (-119.5)- (-150.4) = -358.5 + 150.4. The enthalpy of combustion of cyclohexane, cyclohexene and \$H_2\$ are respectively -3920, -3800 and -241 kJ/mol. The enthalpy of hydrogenation of cyclohexene is -119.5 kJ mol, Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are -382.64 kJ mol^-1, The enthalpy and entropy change for the reaction: Br2(l) + Cl2(g) → 2BrCl(g) are 30 kJ mol^-1. Thus, heat of hydrogenation of 1-butene is -30.3 kcalmol-1. Study Forum Helper; Badges: 17.  d.i. C6H10 + H2 -> C6H12 HӨ = –120 kJ mol–1 Calculate the enthalpy change of hydrogenation of benzene to cyclohexane, assuming it has the cyclohexatrienestructure (b) The experimental value for the hydrogenation of benzene to cyclohexane is –207 kJ mol–1. The percentage difference between these two methods (average bond enthalpies and enthalpies of combustion) is greater for cyclohexene than it was for ethene. 0. reply. 4 k J m o l − 1 , its enthalpy of hydrogenation would be: A The enthalpy of hydrogenation of cyclohexene is -119.5kJ/mol. Enthalpy of hydrogenation of one mole benzene to cyclohexane is :