a$.$ As the example on the page $8$ in chapter $2$ slides, yet now the condition is changed

to $1$ mole water at $40C$ placed in a room at $25C.$ What will the entropy of the

system $($water$)$ change after infinite time, when $T$ of the water is equal to

surrounding? Although the entropy change of the system is negative, the process is

still spontaneous, why?

b$.$ Set the total entropy $($system $+$ surrounding$)$ when the water temperature is equal to

surrounding as $\text{'}0\text{'}.$ Please draw the relationship between total entropy and water

temperature $(1040C).$ You can set the y $-$axis as total entropy and x $-$axis as the

water T$.$ The diagram should be drawn with program, such as Excel, MATLAB,

Origin, etc. Hand$-$drawn figures aren't acceptable.