At standard conditions, if the change in the enthalpy for the following reaction is –109 kJ ${\mathrm{mol}}^{-1}$.
${\mathrm{H}}_{2\left(\mathrm{g}\right)} + {\mathrm{Br}}_{2\left(\mathrm{g}\right)} \to 2{\mathrm{HBr}}_{\left(\mathrm{g}\right)}$
Given that bond energy of ${\mathrm{H}}_2$ and ${\mathrm{Br}}_2$ is
435 kJ ${\mathrm{mol}}^{-1}$ and 192 kJ ${\mathrm{mol}}^{-1}$, respectively,
what is the bond energy (in kJ ${\mathrm{mol}}^{-1}$) of HBr?