One mole of water is placed in surroundings at -3 °C, but at first it does not freeze (it remains as supercooled water). Suddenly it freezes. Calculate the entropy change in the system during the freezing, making use of the following data: CP„(water)=75.3JK'mol Cp„(ice)=37.7JK-mol¬ A,H(ice→water)=6.02kJ mol' at 0 °C The two Cp values can be assumed to be independent of temperature. Also, calculate the entropy change in the surroundings, and the net entropy change in the system and surroundings.
One mole of water is placed in surroundings at -3 °C, but at first it does not freeze (it remains as supercooled water). Suddenly it freezes. Calculate the entropy change in the system during the freezing, making use of the following data: CP„(water)=75.3JK'mol Cp„(ice)=37.7JK-mol¬ A,H(ice→water)=6.02kJ mol' at 0 °C The two Cp values can be assumed to be independent of temperature. Also, calculate the entropy change in the surroundings, and the net entropy change in the system and surroundings.
Chapter4: The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 4.7CYU: Check Your Understanding A 50-g copper piece at a temperature of 20 is placed into a large...
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