The average bond enthalpy for C__H is 413 kJ/mol. In other words, 413 kJ of energy is required to break a mole of CH into atoms:

CH (g) ----> C(g) + H(g) delta H= 413 kJ

Using this information, and enthalpy of C6H6=5535kJ, calculate the enthalpy change of the reaction:
C6H6 (g) --> 6CH (g)

To calculate the enthalpy change of the reaction, we need to use the concept of bond enthalpy. The enthalpy change of a reaction can be calculated by summing up the bond energies of the bonds broken, and subtracting the sum of the bond energies of the bonds formed.

Given the average bond enthalpy for C__H is 413 kJ/mol, we can calculate the energy required to break all the bonds in C6H6 (g):
6 mol of C__H bonds are broken in the reaction C6H6 (g) --> 6CH (g)
Energy required to break the bonds in C6H6 = 6 mol x 413 kJ/mol = 2478 kJ

Now, we need to determine the energy released when 6 CH (g) bonds are formed:
The given enthalpy of C6H6 is 5535 kJ.
From the equation, we can see that 6 CH (g) bonds are formed when one mole of C6H6 is decomposed.
Therefore, energy released when 6 CH (g) bonds are formed = 5535 kJ/mol

Finally, we can calculate the enthalpy change of the reaction by subtracting the energy required to break the bonds from the energy released when the new bonds are formed:
Enthalpy change of the reaction = Energy released - Energy required
Enthalpy change of the reaction = 5535 kJ - 2478 kJ

Thus, the enthalpy change of the reaction C6H6 (g) --> 6CH (g) is 3057 kJ.