The entropy function of a system is given by S(E)= aE(E, – E) where a and E, are positive constants. The temperature of the system is (a) negative for some energies (b) increases monotonically with energy (c) decreases monotonically with energy (d) Zero

Pressure is applied isothermally to a container that holds a liquid. Assuming the liquid is compressible, what has happened to the entropy? The entropy has decreased because the applied pressure results in the particles being less free to move, making their positions more predictable. The entropy has increased because the applied pressure results in heat being transferred from the environment to the system. The entropy has increased because the particles move more rapidly at higher pressure, making their velocities less predictable. None of the above.

A high temperature reservoir losing heat and hence entropy is a reversible process. A low temperature reservoir gaining a certain amount of heat and hence entropy is a reversible process. But a high temperature reservoir losing heat to a low temperature reservoir is irreversible. Why?

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