Hydrogen bromide breaks down to produce hydrogen and bromine: $2\text{HBr(g)} \rightarrow \text{H}_2\text{(g)} + \text{Br}_2\text{(g)}$. The bond energies are provided. What is the energy change for this reaction?
- A$+263\,\text{kJ mol}^{-1}$
- B$+103\,\text{kJ mol}^{-1}$
- C$-103\,\text{kJ mol}^{-1}$
- D$-263\,\text{kJ mol}^{-1}$