Carbon monoxide and methanol may react together to produce ethanoic acid. $\text{CO}(g) + \text{CH}_3\text{OH}(l) \xrightarrow[]{\Delta H^{\circ}} \text{CH}_3\text{CO}_2\text{H}(l)$ The table lists the standard enthalpy changes of combustion. $\Delta H_c^{\circ}(\text{CO}) = -283.0\,\text{kJ mol}^{-1}$ $\Delta H_c^{\circ}(\text{CH}_3\text{OH}) = -726.0\,\text{kJ mol}^{-1}$ $\Delta H_c^{\circ}(\text{CH}_3\text{CO}_2\text{H}) = -874.1\,\text{kJ mol}^{-1}$ Determine the value of $\Delta H_r^{\circ}$ for the reaction between carbon monoxide and methanol?
- A$-1883.1\,\text{kJ mol}^{-1}$
- B$-134.9\,\text{kJ mol}^{-1}$
- C$+134.9\,\text{kJ mol}^{-1}$
- D$+1883.1\,\text{kJ mol}^{-1}$