A table provides some bond energy data. Hydrazine, $\text{N}_2\text{H}_4$, reacts with oxygen, as shown. $\text{N}_2\text{H}_4 + \text{O}_2 \rightarrow 2\text{H}_2\text{O} + \text{N}_2$. The enthalpy change, $\Delta H$, for this reaction is found by choosing and applying data from the table. What is the value of $\Delta H$?
- A$-728\,\text{kJ/mol}$
- B$-568\,\text{kJ/mol}$
- C$-34\,\text{kJ/mol}$
- D$+352\,\text{kJ/mol}$