Use the bond energy data and calculate the enthalpy change for the above reaction. The bond energies of C-H and C-Cl are 413 and 328 kJ/ mol respectively.

(a)- 1428 kJ/ mol
(b)- -1428 kJ/ mol
(c)- 2482 kJ/ mol
(d)- -2482 kJ/ mol

Hint: To calculate the change in enthalpy of the reaction, take the difference of the bond energies of the reactant and bond energies of the product. If there is no bond in reactant or product then, take the value as 0.

Complete answer:
We know that in the reaction, the reactant molecule combines with each other or there is a breaking of bond and the products are formed. New bonds are formed in products. Energy is either released or absorbed when the bond breaks or forms. With the help of bond energies, we can calculate the enthalpy of the reaction.
To calculate the change in enthalpy of the reaction, take the difference of the bond energies of the reactant and bond energies of the product. This can be written as:
$\Delta H=\sum{\text{Bond energy}{{\text{y}}_{R}}}-\sum{\text{Bond energy}{{\text{y}}_{P}}}$
The given reaction in the question is:

As we can see that there is no bond on the reactant side, so we have to take the value of bond energy as 0 for the reactant. On the product side, there are two C-H bonds and two C-Cl bonds, by adding their values, we get the bond energy of the product.
Now, putting all the values, we get:
$\Delta H=0-(413+413+328+328)=-1482$
So, the change in the enthalpy of the reaction is -1482 kJ/ mol.

Therefore, the correct answer is an option (b).

Note:
You have to add the bond energies of all the bonds present in the reaction. Sometimes, aromatic rings are given in the condensed form, so open all the structures which will help to calculate the correct bond energy.