Question #3ae78

1 Answer
Sep 2, 2016

Answer:

#DeltaH=193(kJ)/(mol)#

Explanation:

The formation of individual bromine atom at a gaseous state #Br(g)# would result from breaking the covalent bond of the bromine molecule #Br_2(g)# according to the following reaction:

#Br_2(g)->2Br(g)" " "DeltaH=193(kJ)/(mol)#

Thus, for this reaction to occur, enough energy should be supplied to break the #Br-Br# bond, which is going to be equal to the #DeltaH_f# of a bromine atom.

So, the bond dissociation energy of a #Br-Br# bond is equal to:

#DeltaH=193(kJ)/(mol)#