Why does ammonium nitrate (nh4no3) dissolve readily in water even though the dissolution process is endothermic by 26.4 kj/mol? why does ammonium nitrate (nh4no3) dissolve readily in water even though the dissolution process is endothermic by 26.4 kj/mol? the vapor pressure of the water decreases upon addition of the solute. the osmotic properties of the system lead to this behavior. the overall enthalpy of the system decreases upon addition of the solute. the overall entropy of the system increases upon dissolution of this strong electrolyte. the overall enthalpy of the system increases upon dissolution of this strong electrolyte.

Option (c) is the correct answer.

Explanation:

Entropy is defined as the degree of randomness that is present within the particles of a substance.

As is ionic in nature. Hence, when it is added to water then it will readily dissociate into ammonium ions () and nitrate ions ().

Therefore, it means that ions of ammonium nitrate will be free to move from one place to another. Hence, there will occur an increase in entropy.

Thus, we can conclude that ammonium nitrate () dissolve readily in water even though the dissolution process is endothermic by 26.4 kJ/mol because the overall entropy of the system increases upon dissolution of this strong electrolyte.

the electronic configuration of an atom with eight electrons is 1s²2s²2p⁴. the orbital diagrams are shown in the figure.

as per the hunds rule:

1. electrons tend to avoid being in the same orbital as per as practicable.

2. electrons in different orbitals of the same energy will have their spin parallel.

this can be illustrated from the multiplicity of the orbitals of the atom. as there are four electrons in the p orbital and p orbital has 3 sub-shells. the electrons can be fed in different ways as shown in the figure but the correct orbital diagram will be as per the hunds rule.