# Question #3ae78

Sep 2, 2016

$\Delta H = 193 \frac{k J}{m o l}$

#### Explanation:

The formation of individual bromine atom at a gaseous state $B r \left(g\right)$ would result from breaking the covalent bond of the bromine molecule $B {r}_{2} \left(g\right)$ according to the following reaction:

$B {r}_{2} \left(g\right) \to 2 B r \left(g\right) \text{ " } \Delta H = 193 \frac{k J}{m o l}$

Thus, for this reaction to occur, enough energy should be supplied to break the $B r - B r$ bond, which is going to be equal to the $\Delta {H}_{f}$ of a bromine atom.

So, the bond dissociation energy of a $B r - B r$ bond is equal to:

$\Delta H = 193 \frac{k J}{m o l}$