Enthalpy of atomisation of diamond is `600 kJ//mol.C` (diamond) `rarrC(g)`. Find the bond energy of `C-C` bond.

Options

A. `30KJ mol`.
B. `3000 KJ//mol`.
C. `15KJ//mol`.
D. None of these

Explanation

To find the bond energy of the C-C bond from the given enthalpy of atomization of diamond, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Concept of Enthalpy of Atomization**:
- The enthalpy of atomization is the energy required to convert one mole of a substance into its gaseous atoms. In this case, we are converting diamond (a solid form of carbon) into gaseous carbon atoms.

2. **Given Data**:
- The enthalpy of atomization of diamond is given as \(600 \, \text{kJ/mol}\).

3. **Identify the Reaction**:
- The reaction can be represented as:
\[ \text{C (diamond)} \rightarrow \text{C (g)} \]
- This reaction involves breaking bonds in the diamond structure to form gaseous carbon atoms.

4. **Determine the Number of C-C Bonds Broken**:
- In diamond, each carbon atom is tetrahedrally bonded to four other carbon atoms. To convert diamond to gaseous carbon, we need to break multiple C-C bonds.
- For one mole of diamond, we break 2 C-C bonds to produce 1 mole of gaseous carbon atoms.

5. **Calculate the Bond Energy**:
- Since the enthalpy change for breaking 2 C-C bonds is \(600 \, \text{kJ}\), the bond energy for one C-C bond can be calculated as:
\[ \text{Bond Energy} = \frac{\text{Enthalpy of Atomization}}{\text{Number of Bonds Broken}} = \frac{600 \, \text{kJ}}{2} = 300 \, \text{kJ/mol} \]

6. **Conclusion**:
- The bond energy of the C-C bond is \(300 \, \text{kJ/mol}\).

### Final Answer:
The bond energy of the C-C bond is \(300 \, \text{kJ/mol}\).

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