The discussion revolves around the concept of standard entropy values, particularly focusing on why certain aqueous ions, like Ca2+, can have negative standard entropy values, and the general observation that pure elements have positive standard entropy values. The scope includes theoretical considerations of entropy in dissolution processes and the underlying interactions involved.
Participants express uncertainty regarding the relationship between dissolution and entropy changes, indicating that multiple competing views remain on the factors influencing standard entropy values. The discussion on the terminology also highlights a lack of consensus on the correct terms being used.
Limitations include potential misunderstandings about the definitions of enthalpy and entropy, as well as the complexities involved in measuring interactions that affect entropy during dissolution.
Start dropping solvent dipoles into an electrical potential well. There's more going on than just entropy of mixing.Conservation said:how is this possible when dissolution is usually an increase in entropy?
Enthalpy? Again, you mean "entropy?" It's the integral of Cp/T from absolute zero to 298 K (or whatever T for the table).Conservation said:elements always having a positive standard enthalpy?