A mixture of 1773 g of water and 227 g of ice is in an initial equilibrium state at 0.000oC. The mixture is then, in a reversible process, brought to a second equilibrium state where the water-ice ratio, by mass, is 1.00: 1.00 at 0.000oC.

(a) Calculate the entropy change of the system during this process. (The heat of fusion for water is 333kJ/kg.)

(b) The system is then returned to the initial equilibrium state in an irreversible process (say by using a Bunsen burner). Calculate the entropy change of the system during this process.

(c) Are your answers consistent with the second law of thermodynamics?