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