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

Explanation

We have
`O_(2) overset(hv) to O_("Normal") + O_("excted")`
`O_(2) rarr+ O_("Normal") + O_("excted")`
Energy required dissociation of `O_(2)` into two normal atoms `= (498 xx 10^(3))/(6.023 xx 10^(22) 1 mol ^(-1)`
If one atom in excited state has energy i.e. `1.967eV = 1.967 xx 1.602 xx 10^(-19) J` , the energy required for photochemical dissociation of `O_(2)` is
`= (498 xx 10^(3))/(6.023 xx 10^(23)) + 1.967 xx 1.67 xx 1.602 xx 10^(-19)`
`= 82 .68 xx 10^(-20) + 31.51 xx 10^(-20)`
`= 114.19 xx 10^(-20) J`
`E = (hc)/(lambda)`
`114.19 xx 10^(-20) = (6.625 xx 10^(-20) xx 3 xx 10^(-8))/(lambda)`
`lambda =- 1740.2 xx 10^(-10) m = 1740.2 Å`