Bond dissociation enthalpy (BDE) is the change in enthalpy, when one mole of identical covalent bonds broken to form free radicals in gas phase. In case of polyatomic molecules bond dissociation enthalpy is different for different bonds within the same molecule. Bond dissociation energy is affected by s orbital character involved in bonding atoms. Use the following data given with uncertainity of $\pm 1 KJ / mole$
$\begin{array}{lr} {Cl}_{2 (g)} \to 2 {Cl}_{(g)} {ΔH}^{0} = 242 kJ / mol \\ {CH}_{4 (g)} \to C_{(g)} + 4 H_{(g)} {ΔH}^{0} = 1665 kJ / mol \\ H_{2} (g) \to 2 H_{(g)} {ΔH}^{0} = 435 kJ / mol \\ {Cl}_{3} C - H_{(g)} \to {Cl}_{3} C_{(g)} + H_{(g)} {ΔH}^{0} = 347 kJ / mol \\ {HCl}_{(g)} \to H_{(g)} + {Cl}_{(g)} {ΔH}^{0} = 431 kJ / mol \\ {Cl}_{3} C - {Cl}_{(g)} \to {Cl}_{3} C_{(g)} + {Cl}_{(g)} {ΔH}^{0} = 431 kJ / mol \end{array}$

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