`O_(2)` undergoes photochemical dissociation into one normal oxygen atom and one excited oxygen atom. Excited oxygen atom is `1.967 eV` more energetic than normal . The dissociation of `O_(2)` into two normal atoms of oxygen required `498 kJ mol^(-1)`, what is the maximum wavelength effective for photochemical dissociation of `O_(2)`?

Explanation

Energy required to break one bond between O-atom `=(498xx10^(3))/(6.023xx10^(23))xx(1)/(1.6xx10^(-19))eV=5.17eV`
Total energy of photon `=5.17eV + 1.967 eV = 7.137 eV`
let `lambda` = wavelength required `implies (hc)/(lambda) =(1240)/(lambda(nm))=7.137eVimplies lambda= (1240)/(7.137)=173.7nm`