Enthalpy of atomisation of a diamond is $600 k J / m o l .$
$C (d i a m o n d) \to C (g) .$
Using this data the bond energy of C-C bond was found to be $x \times 10^{2} k J / m o l$ where x is an interger between 0 to 9. Value of x is

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Solution

In producing one mole of C(g).
number $C - C$ bonds broken = $\frac{1}{2} \times 4 \times N_{A} = 2 N_{A}$
So $2 N_{A} C - C$ bonds contain energy equal to energy of atomisation.
but energy of atomisation is $600 k J / m o l .$

comparing the values,
$2 N_{A} ϵ_{C - C} = 600 k J$
$2 N_{A} ϵ_{C - C} = \frac{300 k J}{N_{A}}$
$ϵ_{C - C} = 300 k J / m o l$

comparing this to question,
clearly, x=3

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Enthalpy of atomisation of a diamond is 600 kJ/mol. C(diamond)→C(g). Using this data the bond energy of C-C bond was found to be x×102 kJ/mol where x is an interger between 0 to 9. Value of x is

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Enthalpy of atomisation of a diamond is $600 k J / m o l .$
$C (d i a m o n d) \to C (g) .$
Using this data the bond energy of C-C bond was found to be $x \times 10^{2} k J / m o l$ where x is an interger between 0 to 9. Value of x is