\textbf{219.} From the decomposition of each gram of ammonium nitrate, according to the reaction (unbalanced):
$$\text{NH}_4\text{NO}_3(s) \rightarrow \text{N}_2(g) + \text{H}_2\text{O}(g) + \text{O}_2(g)$$
$1.5\ \text{kJ}$ of energy is released. If the enthalpy of formation of $\text{H}_2\text{O}(g)$ is $-245\ \text{kJ.mol}^{-1}$, what is the enthalpy of formation of ammonium nitrate per mole?
$(H = 1,\ N = 14,\ O = 16 : \text{g.mol}^{-1})$
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(1) $-370$ \hfill (2) $+370$ \hfill (3) $-440$ \hfill (4) $+440$
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