The change in specific enthalpy during melting of ice at 0 C and 1.01 bar is 333

Question

The change in specific enthalpy during melting of ice at 0 C and 1.01 bar is 333.39 kJ/kg. Given a system consisting of ice and liquid water at 0 C and 1.01 bar in thermal contact with an environment at 20 C, find for the process of melting 2 kg of ice at 0 C at 1.01 bar the entropy change (kJ/K) of (a) the ice, (b) the environment, and (c) the universe (ice and environment). Note: The ice-liquid water system is closed so the enthalpy change is not directly related to the heat transfer. However, from the fundamental definition of an enthalpy change (?h = ?u + ?pV), and from the facts that ice and water are incompressible and the process is at constant pressure, the enthalpy of melting can be easily transformed into the appropriate internal energy quantity.

Explanation / Answer

a) Entropy chnage of ice = 2*333.39/(273+0) = 2.442 kJ/K b) Entropy change of env = -2*333.39/(20+273) = -2.276 kJ/K c) Entropy change of universe = 2.442 + (-2.276) = 0.166 kJ/K

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