The information below is required for this question. $\Delta H_f^\circ(\text{N}_2\text{H}_4(\ell)) = 50.6\,\text{kJ mol}^{-1}$, $\Delta H_f^\circ(\text{N}_2\text{O}_4(\text{g})) = 9.2\,\text{kJ mol}^{-1}$, $\Delta H_f^\circ(\text{H}_2\text{O}(\text{g})) = -241.8\,\text{kJ mol}^{-1}$. Hydrazine, $\text{N}_2\text{H}_4(\ell)$, combines with dinitrogen tetraoxide, $\text{N}_2\text{O}_4(\text{g})$, producing nitrogen gas and water vapour: $2\text{N}_2\text{H}_4(\ell) + \text{N}_2\text{O}_4(\text{g}) \rightarrow 3\text{N}_2(\text{g}) + 4\text{H}_2\text{O}(\text{g})$. What is the enthalpy change for this reaction?
- A$-1077.6\,\text{kJ mol}^{-1}$
- B$-856.8\,\text{kJ mol}^{-1}$
- C$-301.6\,\text{kJ mol}^{-1}$
- D$-182.0\,\text{kJ mol}^{-1}$