17.1 Introduction to Entropy; Intuition on Signs of Entropy Changes

Enthalpy is insufficient to explain spontaneity. Entropy as randomness, disorder, or energy dispersal. Sign changes for Delta S in phase-change processes and chemical reactions. Sign changes for Delta S in dissolution processes.

00:00 Enthalpy Change and Spontaneity
00:54 Entropy is a Measure of Energy Dispersal
02:47 Units of Entropy; Classical Entropy as a Concept
05:29 Entropy and Phase
07:43 Entropy Changes in Gaseous Chemical Reactions
09:02 Entropy Changes in Dissolution Processes

[SilentSnipest]

I'm a bit confused by the delta S being lower at higher T and delta S being greater at lower T. Your stadium example makes perfect sense, but I always thought the increased temperature would allow for molecules to more easily disperse due to increased kinetic energy. That can be seen in your solid-> liquid-> gas figure. Wouldn't this increased T result in increased randomness (thus a greater change in entropy)?

Edit: Oh, were you talking specifically about when you introduce a new chamber to your system that has a greater T? So your fixed heat value has less entropy change overall because your other system already had a lot of internal energy and was already quite dispersed? Something about that example is confusing me.