Suppose you put 2.00 kg of pure liquid water, initially at 0.00°C, in a room. The temperature of the room is T room= −10.0 ° C . Assume the system of the room plus the water is thermally isolated, i.e. a closed system. Lf , water=3.34×10^5 J/kg The process you will be analyzing is the following: The water transfers heat into the room, such that the water freezes to form a 2.00 kg block of pure ice, still at 0.00°C. The room is large enough that its temperature remains constant at -10.0°C during this process. a) Find the change in the entropy of the water/ice during this process. b) Find the change in the entropy of the room during this process. c) Comment on the likelihood that this freezing process will occur, using the ideas of the Second Law of Thermodynamics and microstates in your explanation
Suppose you put 2.00 kg of pure liquid water, initially at 0.00°C, in a room. The temperature of the room is T room= −10.0 ° C . Assume the system of the room plus the water is thermally isolated, i.e. a closed system. Lf , water=3.34×10^5 J/kg
The process you will be analyzing is the following: The water transfers heat into the room, such that the water freezes to form a 2.00 kg block of pure ice, still at 0.00°C. The room is large enough that its temperature remains constant at -10.0°C during this process.
a) Find the change in the entropy of the water/ice during this process.
b) Find the change in the entropy of the room during this process.
c) Comment on the likelihood that this freezing process will occur, using the ideas of the Second Law of
Step by step
Solved in 3 steps
