Bond enthalpy

Match List - I with List - II.

Choose the correct answer from the options given below :

Correct match of the C-H bonds (shown in bold) in Column J with their BDE in Column K is

Column J: Molecule	Column K: BDE (kcal mol$^{-1}$)
(P) $\mathbf{H{-}C}\mathrm{H(CH_3)_2}$	(i) 132
(Q) $\mathbf{H{-}C}\mathrm{H_2Ph}$	(ii) 110
(R) $\mathbf{H{-}C}\mathrm{H{=}CH_2}$	(iii) 95
(S) $\mathbf{H{-}C}{\equiv}\mathrm{CH}$	(iv) 88

For the following reaction
$$\ce{CH4(g) + Cl2(g) ->[light] CH3Cl(g) + HCl(g)}$$
the correct statement is

The heat of atomization of methane and ethane are 360 kJ/mol and 620 kJ/mol, respectively. The longest wavelength of light capable of breaking the C - C bond is (Avogadro number = $6.02\times10^{23}$, $h=6.62\times10^{-34}$ J s) :

The standard enthalpy of formation of $\ce{NH3}$ is $-46.0$ kJ/mol. If the enthalpy of formation of $\ce{H2}$ from its atoms is $-436$ kJ/mol and that of $\ce{N2}$ is $-712$ kJ/mol, the average bond enthalpy of N-H bond in $\ce{NH3}$ is :

The standard enthalpy of formation ($\Delta_fH^\circ_{298}$) for methane, $\ce{CH4}$ is $-74.9$ kJ mol$^{-1}$. In order to calculate the average energy given out in the formation of a C−H bond from this it is necessary to know which one of the following ?

Using the data provided, calculate the multiple bond energy (kJ mol⁻¹) of a C≡C bond in $\ce{C2H2}$. That energy is (take the bond energy of a C-H bond as 350 kJ mol⁻¹.)

$\ce{2C(s) + H2(g) -> C2H2(g)}$, $\Delta H=225$ kJ mol⁻¹

$\ce{2C(s) -> 2C(g)}$, $\Delta H=1410$ kJ mol⁻¹

$\ce{H2(g) -> 2H(g)}$, $\Delta H=330$ kJ mol⁻¹

The bond energy (in kcal mol⁻¹) of a C-C single bond is approximately