Final answer:
The enthalpy of solution for ammonium nitrate being positive means that |ΔHsolute| is greater than |ΔHhydration|, as the overall process absorbs heat indicating an endothermic reaction with high lattice energy.
Step-by-step explanation:
The enthalpy of solution, ΔHsoln, for ammonium nitrate is +25.7 kJ/mol. This represents the net energy change when 1 mole of ammonium nitrate dissolves in water. Since the enthalpy of solution is positive, it indicates the process is endothermic, meaning that it absorbs heat from its surroundings. The equation for enthalpy of solution is: ΔHsoln = ΔHsolute + ΔHhydration.
Given that the enthalpy of solution is positive, we can conclude that the enthalpy of solute breaking (also known as lattice energy), |ΔHsolute|, is greater than the enthalpy of hydration, |ΔHhydration|, which is the energy released when the ions interact with water molecules. This can be symbolized as |ΔHsolute| > |ΔHhydration|, because the process of dissolving is endothermic overall.