The equation representing the combustion of methane is given below. $\text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O}$ The energy change for the combustion of methane is $-890\,\text{kJ mol}^{-1}$. The bond energies are listed in the table. What is the bond energy of the C=O bond?
- A$+49\,\text{kJ mol}^{-1}$
- B$+841\,\text{kJ mol}^{-1}$
- C$+1301\,\text{kJ mol}^{-1}$
- D$+1335\,\text{kJ mol}^{-1}$