Ammonium nitrate (NH₄NO₃) dissolves readily in water even though the dissolution is endothermic by 26.4 kJ/mol. The solution process is spontaneous because _. A) of the increase in disorder upon dissolution of this strong electrolyte B) the vapor pressure of the water decreases upon addition of the solute C) of the increase in enthalpy upon dissolution of this strong electrolyte D) of the decrease in enthalpy upon addition of the solute E) osmotic properties predict this behavior

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Quizplus · Accepted Answer

The dissolution of ammonium nitrate is spontaneous because of the increase in disorder (or entropy) upon dissolution of this strong electrolyte. When ammonium nitrate dissolves in water, its ions dissociate and become surrounded by water molecules, which leads to an increase in the randomness of the system. This increase in entropy is able to overcome the endothermic nature of the dissolution, making the process spontaneous.

Ammonium Nitrate (NH4NO3) Dissolves Readily in Water Even Though the Dissolution

Ammonium Nitrate (NH₄NO₃) Dissolves Readily in Water Even Though the Dissolution