`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

To solve the problem of finding the maximum wavelength effective for the photochemical dissociation of \( O_2 \), we will follow these steps:

### Step 1: Understand the Energy Requirements
We know that the dissociation of \( O_2 \) into two normal oxygen atoms requires \( 498 \, \text{kJ/mol} \). Additionally, one of the oxygen atoms is excited and has an energy of \( 1.967 \, \text{eV} \) more than the normal oxygen atom.

### Step 2: Convert Energy from kJ/mol to Joules
To work with consistent units, we need to convert the dissociation energy from kJ/mol to Joules.

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