The equation below represents the complete combustion of methane. $\text{CH}_4\text{(g)} + 2\text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} + 2\text{H}_2\text{O( g)}$ The bond energies are listed in the table. What is the energy change for this reaction?
- A$-818\,\text{kJ mol}^{-1}$
- B$-359\,\text{kJ mol}^{-1}$
- C$-323\,\text{kJ mol}^{-1}$
- D$+102\,\text{kJ mol}^{-1}$