The amount of energy required to break a bond is same as the amount of energy released when the same bond is formed. In gaseous state, the energy required for homolytic cleavage of a bond is called Bond Dissociation Energy (BDE) or Bond Strength. BDE is affected by s-character of the bond and the stability of the radicals formed. Shorter bonds are typically stronger bonds. BDEs for some bonds are given below : $Cl$ $-$ $Cl$ (g) $\to$ $Cl$ ${}_{(g)}^ \bullet$ + $Cl$ ${}_{(g)}^ \bullet \Delta$ H ${}^\circ$ = 58 kcal mol $-$ 1 $H_3C$ $-$ $Cl$ (g) $\to$ $H_3C$ ${}_{(g)}^ \bullet$ + $Cl$ ${}_{(g)}^ \bullet \Delta$ H ${}^\circ$ = 85 kcal mol $-$ 1 $H$ $-$ $Cl$ (g) $\to$ $H$ ${}_{(g)}^ \bullet$ + $Cl$ ${}_{(g)}^ \bullet \Delta$ H ${}^\circ$ = 103 kcal mol $-$ 1For the following reaction $CH_4$(g) + $Cl_2$(g) $\xrightarrow{light}$ $CH_3Cl$(g) + $HCl$ (g) the correct statement is