# Why is the change in entropy greater for processes occurring at lower temperatures? [duplicate]

We have the thermodynamic definition of entropy $\Delta S = q_{rev}/T$. If heat transfer is the same for both processes at different temperatures, this implies that the same process occurring at lower temperature would generate more entropy than if the process occurred at higher temperature. Why is this the case? Why isn't the change in entropy equal for both processes?

• – Gert Nov 1 '15 at 2:49
• I'm looking for an intuitive explanation rather than a mathematical one... – notorious Nov 1 '15 at 4:15
• In many cases, this formula (or the equivalent in terms of Carnot processes) is taken as the definition of (absolute) temperature. If you want an explanation of this formula, you have to tell us how you want to define temperature in the first place... – Fabian Nov 1 '15 at 21:13
• You might be able to avoid this getting closed as a duplicate if you make it explicit that you want an intuitive picture rather than equations. Still, as noted by @Gert, this really was asked already and has a reasonably good answer. – DanielSank Nov 3 '15 at 9:32
• The second link (Why does heat added to a system...) explicitly asks for intuition. – user10851 Nov 9 '15 at 7:39