Methanol can be produced by allowing carbon monoxide to react with hydrogen. $\text{CO(g)} + 2\text{H}_2\text{(g)} \rightarrow \text{CH}_3\text{OH(g)}$ The average bond energies needed are listed below. $E(\text{C} \equiv \text{O}) = 1077\,\text{kJ mol}^{-1}$ $E(\text{C-O}) = 360\,\text{kJ mol}^{-1}$ $E(\text{C-H}) = 410\,\text{kJ mol}^{-1}$ $E(\text{H-H}) = 436\,\text{kJ mol}^{-1}$ $E(\text{O-H}) = 460\,\text{kJ mol}^{-1}$ Calculate the enthalpy change for this reaction.
- A$-537\,\text{kJ mol}^{-1}$
- B$-101\,\text{kJ mol}^{-1}$
- C$+101\,\text{kJ mol}^{-1}$
- D$+537\,\text{kJ mol}^{-1}$