When ammonium nitrate dissolves in water and the temperature of the surroundings drops, it indicates that the dissolution process is endothermic. In an endothermic process, energy is absorbed from the surroundings, leading to a decrease in the temperature of the surroundings.
In terms of potential energy, this dissolution implies the following:
The potential energy of ammonium nitrate is higher when it is a solid than when it dissolves.
This is because, during the dissolution process, the solid form of ammonium nitrate (with its structured lattice) breaks apart, and energy is absorbed to overcome the lattice energy and allow the ions to disperse in solution. Therefore, the potential energy is higher in the solid state compared to the dissolved state.
Thus, the correct response is:
The potential energy of ammonium nitrate is higher when it is a solid than when it dissolves.
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