An energy cycle is shown for this reaction. $\text{Br}_2(\text{l}) + 3\text{F}_2(\text{g}) \rightarrow 2\text{BrF}_3(\text{l})$ The standard enthalpy of formation of $\text{BrF}_3(\text{l})$ is $-301\,\text{kJ mol}^{-1}$. The enthalpy change from $\text{BrF}_3(\text{l})$ to $\text{BrF}_3(\text{g})$ is $+44\,\text{kJ mol}^{-1}$. What is the average bond energy of the 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$404\,\text{kJ mol}^{-1}$