At 298K, NH4NO3 readily dissolves in water, suggesting that the change in free energy (ΔG) favors the dissolution process. However, when NH4NO3 dissolves in water, the temperature of the water decreases. The particulate diagram above attempts to provide a microscopic view of the dissolution of NH4NO3(s) considering both the change in enthalpy (ΔH) and the change in entropy (ΔS). Which of the following explains what the particle diagram is able to illustrate and why? A) The particle diagram is able to illustrate that the ΔH for the dissolution of NH4NO3 is exothermic because overcoming the attractive forces between the ions requires the absorption of energy.

B) The particle diagram is able to illustrate that the ΔH for the dissolution of NH4NO3 is endothermic because forming new interactions between the ions and the water molecules releases energy.

C) The particle diagram is able to illustrate that entropy increases when NH4NO3(s) dissolves in water because the ions disperse in solution.

D) The particle diagram is able to illustrate that entropy decreases when NH4NO3(s) dissolves in water because many hydrogen bonds can form between the water molecules and the ions.