The dissolution of ammonium chloride in water is an endothermic process but still it dissolves in water readily. Why?
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This is because of entropy change. In this case, $\Delta\text{S}$ is +ve.$\text{NH}_4\text{Cl}(\text{aq})\rightarrow\text{NH}^+_4+\text{Cl}^-(\text{aq})$
The ions that were held together in crystalline solid are free and moving in all possible directions. Its entropy has increased and this makes $\text{T}\Delta\text{S}>\Delta\text{H},\ \text{i.e., }\Delta\text{G}=-\text{ve}.$
The ions that were held together in crystalline solid are free and moving in all possible directions. Its entropy has increased and this makes $\text{T}\Delta\text{S}>\Delta\text{H},\ \text{i.e., }\Delta\text{G}=-\text{ve}.$
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