An energy cycle diagram is shown for this reaction. $\text{Br}_2(l) + 3\text{F}_2(g) \rightarrow 2\text{BrF}_3(l)$ The standard enthalpy of formation of $\text{BrF}_3(l)$ is $-301\,\text{kJ mol}^{-1}$. The enthalpy change for $\text{BrF}_3(l)$ changing to $\text{BrF}_3(g)$ is $+44\,\text{kJ mol}^{-1}$. Calculate the average bond energy of the $\text{Br--F}$ bond in $\text{BrF}_3$?
- A$152\,\text{kJ mol}^{-1}$
- B$202\,\text{kJ mol}^{-1}$
- C$304\,\text{kJ mol}^{-1}$
- D$404\,\text{kJ mol}^{-1}$