The reaction equation for hydrogen reacting with chlorine is shown below. $\text{H}_2(g) + \text{Cl}_2(g) \rightarrow 2\text{HCl}(g)$ This reaction gives out heat. The bond energies are listed in the table. $\text{Cl--Cl}$: $+240\ \text{kJ mol}^{-1}$ $\text{H--Cl}$: $+430\ \text{kJ mol}^{-1}$ $\text{H--H}$: $+436\ \text{kJ mol}^{-1}$ Determine the energy change for this reaction.
- A$-1536\ \text{kJ mol}^{-1}$
- B$-184\ \text{kJ mol}^{-1}$
- C$+184\ \text{kJ mol}^{-1}$
- D$+246\ \text{kJ mol}^{-1}$