Ammonia \(\left(\mathrm{NH}_{3}\right)\) boils at \(-33^{\circ} \mathrm{C} ;\) at
this temperature it has a density of \(0.81 \mathrm{~g} / \mathrm{cm}^{3}\). The
enthalpy of formation of \(\mathrm{NH}_{3}(g)\) is \(-46.2 \mathrm{~kJ} /
\mathrm{mol}\), and the enthalpy of vaporization of \(\mathrm{NH}_{3}(l)\) is
\(23.2 \mathrm{~kJ} / \mathrm{mol}\). Calculate the enthalpy change when \(1
\mathrm{~L}\) of liquid \(\mathrm{NH}_{3}\) is burned in air to give
\(\mathrm{N}_{2}(g)\) and \(\mathrm{H}_{2} \mathrm{O}(g)\). How does this compare
with \(\Delta H\) for the complete combustion of \(1 \mathrm{~L}\) of liquid
methanol \(\mathrm{CH}_{3} \mathrm{OH}(l) ?\) For \(\mathrm{CH}_{3}
\mathrm{OH}(\mathrm{l})\), the density at \(25^{\circ} \mathrm{C}\) is
\(0.792 \mathrm{~g} / \mathrm{cm}^{3}\), and \(\Delta H_{f}^{\circ}\) equals \(-239
\mathrm{~kJ} / \mathrm{mol}\).