Entropy change, $\Delta{S}$, can be found from the $\frac{1}{T} - Q$ graph. When the temperature doesn't change during the dispersal of heat energy in the system, the area under the graph is more, that is, change in entropy is more. But, when the temperature increases, the area under the graph decreases, that is, change in entropy is less.
I have taken $Q$ on the x-axis and as $T$ is a function of $Q$, $\dfrac{1}{T}$ is represented on the y-axis. Now, when $T$ doesn't change, the graph covers a rectangular area but when $T$ increases, the graph covers much smaller area. So, what's the reason? Do the number of possible microstates decrease when the temperature decreases?
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