Photochemical dissociation of oxygen result in the production of two oxygen atoms one in the ground state and in the excited state
`O_(2) overset(hv) to O + O^(*)`
The maximum wavelength (1) needed for this is `17.4` nm .If the exchation energy `O rarr O^(*) is 3.15 xx 10^(-19) J` How much energy in kJ `mol^(-1)` is needed for the dissociation of `1` mole of oxygen into normal atoms in the ground state

Explanation

To solve the problem, we need to calculate the energy required for the dissociation of one mole of oxygen (O2) into normal oxygen atoms (O) in the ground state. The process involves a few steps, which we will outline below.

### Step-by-Step Solution:

1. **Understanding the Reaction**:
The photochemical dissociation of oxygen can be represented as:
\[
O_2 \overset{hv}{\rightarrow} O + O^*
...