JEE Advanced 2021 — Paper 2 — Question 40

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:

$$\ce{H3C-H(g) -> H3C^{\bullet}(g) + H^{\bullet}(g)} \qquad \Delta H^\circ = 105\ \text{kcal\; mol}^{-1}$$ $$\ce{Cl-Cl(g) -> Cl^{\bullet}(g) + Cl^{\bullet}(g)} \qquad \Delta H^\circ = 58\ \text{kcal\; mol}^{-1}$$ $$\ce{H3C-Cl(g) -> H3C^{\bullet}(g) + Cl^{\bullet}(g)} \qquad \Delta H^\circ = 85\ \text{kcal\; mol}^{-1}$$ $$\ce{H-Cl(g) -> H^{\bullet}(g) + Cl^{\bullet}(g)} \qquad \Delta H^\circ = 103\ \text{kcal\; mol}^{-1}$$

For the following reaction $\mathrm{CH}_{4}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \xrightarrow{\text { light }} \mathrm{CH}_{3} \mathrm{Cl}(\mathrm{g})+\mathrm{HCl}(\mathrm{g})$ The correct statement is