State the balanced equation and enthalpy change, $\Delta H$, for the complete combustion of butanol, $\text{C}_4\text{H}_9\text{OH}$.
- A$\text{C}_4\text{H}_9\text{OH}(l) + 5\text{O}_2(g) \rightarrow 4\text{CO}_2(g) + 5\text{H}_2\text{O}(g)$, $\Delta H = -2676\,\text{kJ mol}^{-1}$
- B$\text{C}_4\text{H}_9\text{OH}(l) + 5\text{O}_2(g) \rightarrow 4\text{CO}_2(g) + 5\text{H}_2\text{O}(g)$, $\Delta H = +2676\,\text{kJ mol}^{-1}$
- C$\text{C}_4\text{H}_9\text{OH}(l) + 6\text{O}_2(g) \rightarrow 4\text{CO}_2(g) + 5\text{H}_2\text{O}(g)$, $\Delta H = -2676\,\text{kJ mol}^{-1}$
- D$\text{C}_4\text{H}_9\text{OH}(l) + 6\text{O}_2(g) \rightarrow 4\text{CO}_2(g) + 5\text{H}_2\text{O}(g)$, $\Delta H = +2676\,\text{kJ mol}^{-1}$