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 :

Options

A. 1168kJ/mol
B. 976kJ/mol
C. 880kJ/mol
D. None of these

Answer

To solve the problem, we need to calculate the total energy required for the dissociation of ozone (O₃) into one normal oxygen atom (O) and one more energetic oxygen atom (O**). The process involves two steps, and we will break down the calculations step by step.

### Step 1: Energy for the dissociation of O₃ into O₂ and O
The first reaction is:
\[ O_3(g) \rightarrow O_2(g) + O(g) \]

According to the problem, the energy required for this dissociation is given as:
\[ \text{Energy required} = 400 \, \text{kJ/mol} \]

### Step 2: Energy for the dissociation of O₂ into O and O**
The second reaction is:
\[ O_2(g) \rightarrow O + O^* \]

The normal dissociation energy of O₂ is given as:
\[ \text{Normal dissociation energy} = 480 \, \text{kJ/mol} \]

Additionally, O** has 1 eV more energy than O, which is equivalent to:
\[ 1 \, \text{eV} = 96 \, \text{kJ/mol} \]

Thus, the total energy required for the dissociation of O₂ into O and O** is:
\[ \text{Total energy for O₂ dissociation} = 480 \, \text{kJ/mol} + 96 \, \text{kJ/mol} = 576 \, \text{kJ/mol} \]

### Step 3: Total energy for the dissociation of O₃ into O and O**
Now, we combine the energies from Step 1 and Step 2 to find the total energy required for the dissociation of O₃ into O and O**:
\[ \text{Total energy} = \text{Energy for O₃ dissociation} + \text{Energy for O₂ dissociation} \]
\[ \text{Total energy} = 400 \, \text{kJ/mol} + 576 \, \text{kJ/mol} = 976 \, \text{kJ/mol} \]

### Final Answer
The total energy required for the dissociation of O₃ into O and O** is:
\[ \boxed{976 \, \text{kJ/mol}} \]