CHM 1046 Lecture Notes - Lecture 39: Enthalpy, Sodium Chloride, Ionic Compound
Document Summary
When two gases dissolve in one another, this cannot be explained by imfs, but only by the increase in entropy. When two different hydrocarbons dissolve in one another, the net change in imfs is vanishing, but they still co-dissolve, because the process involves an increase in entropy. Entropy of specific processes related to solutions (examples): Solids (such as nacl) tend to be highly organized, so breaking them apart represents a huge increase in entropy. If the solvent organizes itself around solute particles (especially when water molecules surround dissolved ions), this process represents a significant decrease in entropy heat and entropy are also. The enthalpy change accompanying one mole of solid ionic compound forming separate gaseous ions. The enthalpy change that accompanies one mole of gases ions dissolving in water to form an infinitely dilute solution. The enthalpy change that accompanies the formation of a solution from a solute and a solvent.
