The discussion centers on the relationship between entropy and heat flow in thermodynamics, specifically referencing the Helmholtz energy and the thermodynamic identity ΔS = ∫dQ/T. It is established that in an open system, the heat flow into the system is influenced by the temperatures and heat capacities of both the system and its surroundings. The confusion arises from the interpretation of entropy; while increased entropy allows for more heat to enter, it does not directly cause more heat to flow into the system. The key takeaway is that as heat enters a system, its entropy increases, not the other way around.
PREREQUISITESStudents of thermodynamics, physicists, and engineers seeking to deepen their understanding of entropy, heat flow, and the principles governing open systems.
I don't think that is what your book says, exactly. Perhaps there is a translation problem because what you have written does not really make any sense. It would make sense if the book said that as heat from the surroundings enters the system, the entropy of the system increases. This is because ΔS = ∫dQ/Taaaa202 said:In my book it says: The bigger entropy of a system, the more heat from the surroundings can enter it. Now, I don't really understand why that is completely. Can anyone explain me? - both in terms of the actual thermodynamic formulas (thermodynamic identity etc.) and in terms of multiplicity?