If the resonance energy of C-H bond is 24.3 kJ/mol the electronegativity difference of C and H is
A 2.08
B 0.65
C 0.50
D 0.36

The ionic resonance energy of C-H bond is ~~ 6.0kcal mol^(-1) . The EN of H is 2.1 . Calculate EN of carbon ? Given : Delta_(C-H) ~~ 6.0 kcal mol^(-1)

The ionic resonance energy of C-H bond is ~~ 6.0kcal mol^(-1) . The EN of H is 2.1 . Calculate EN of carbon ? Given : Delta_(C-H) ~~ 6.0 kcal mol^(-1)

What would be the bond formation energy of C-H bond if its bond energy is + 416.18 kJ mol^(-1) ?

The bond dissociation energy depends upon the nature of the bond and nature of the molecule. If any molecule more than 1 bonds of similar nature are present then the bond energy reported is the average bond energy. If enthalpy of hydrogenation of C_(6)H_(6(l)) "into" C_(6)H_(12(l)) " is " -205 kJ and resonance energy of C_(6)H_(6(l)) is -152kJ//mol then enthalpy of hydrogenation of is ? Answer Delta H_("vap") " of " C_(6)H_(6(l)), C_(6)H_(10(l)), C_(6)H_(12(l)) all are equal:

Bond energies can be obtained by using the following relation: DeltaH (reaction) = sum Bond energy of bonds, broken in the reactants -sum Bond energy fo bonds, formed in the products Bond enegry depends on three factors: a. Greater is the bond length, lesser is the bond enegry. b. Bond energy increases with the bond multiplicity. c. Bond enegry increases with electronegativity difference between the bonding atoms. Use the bond enegries to estimate DeltaH for this reaction: H_(2)(g) +O_(2)(g) rarr H_(2)O_(2)(g) {:("Bond","Bond energy"),(H-H,436 kJ mol^(-1)),(O-O,142 kJ mol^(-1)),(O=O, 499kJ mol^(-1)),(H-O,460kJ mol^(-1)):}

The enthalpy change (DeltaH) for the process, N_(2)H_(4)(g)to 2N(g)+4H(g) is is 1724 kJ mol^(-1) . If the bond energy of N-H bond in ammonia is 391 kJ mol^(-1) , what is the bond energy for N-N bond in N_(2)H_(4) ?

Average C – H bond energy is 416 kJ mol^(-1) . Which of the following is correct?

Calculate the bond energy of C - H bond, given that the heat of formation of CH_4 , heat of sublimation of carbon and heat of dissociation of H_2 are -74.8 + 719.6 and 435 kJ mol^(-1) respectively.

Calculate the enthalpy of combustion of benzene (l) on the basis of the following data: a. Resonance energy of benzene (l) =- 152 kJ// mol b. Enthalpy of hydrogenation of cyclohexene (l) =- 119 kJ//mol c. Delta_(f)H^(Theta)C_(6)H_(12)(l) =- 156 kJ mol^(-1) d. Delta_(f)H^(Theta) of H_(2)O(l) =- 285.8 kJ mol^(-1) e. Delta_(f)H^(Theta)of CO_(2)(g) =- 393.5 kJ mol^(-1)

Using data (all values are in kilocalorie per mole at 25^(@)C ) given below, calculate the bond energy of C-C and C-H bonds. DeltaH^(Theta) combustion of ethane =- 372.0 DeltaH^(Theta) combustion of propane =- 530.0 DeltaH^(Theta) for C ( garphite) rarr C(g) =+ 172.0 Bond enegry of H-H bond =+ 104.0 Delta_(f)H^(Theta) of H_(2)O(l) =- 68.0 Delta_(f)H^(Theta) of CO_(2)(g) =- 94.0