Ozone in the upper atmoshphere absorbs ultraviolet radiation which induces the following chemical reaction `O_(3)(g)rightarrowO_(2)(g)+O(g)` `O_(2)` produced in the above photochemical dissociation undergoes further dissociation into one normal oxygen atom (O) and more energetic oxygen atom `O**`. `O_(2)(g) rightarrowO+O**` `(O**)` has 1 eV more energy than(O) and normal dissociation energy of `O_(2)` is 480 kJ `"mol"^(-1)`. [1 eV/Photon =96 kJ `"mol"^(-1)`] If dissociation of `O_(3)` into `O_(2)` and O requires 400kJ `mol^(-1)` and O_(2) produced in this reaction is further dissociated to O and `O**` then the total energy required to for the dissociation of `O_(3)` into O and `O**` is :
