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1. Observe an ice cube or hold one in your hand. This is water in a solid form, so it has a high structural order. This means that the molecules cannot move very much and are in a fixed position. The temperature of the ice is zero degrees celcius. As a result, the entropy of the system is low.
2. Allow the ice to melt at room temperature. What is the state of molecules in the liquid water now? How did the energy transfer take place? Is the entropy of the system higher or lower? Why?
3. If you were to heat the melted water to its boiling point, what would happen to the entropy of the system?
Part 2:
Think about the world around you. Give another every day example of entropy and explain how it relates to increasing disorder of energy. If all energy tends to become more disordered, how do we always have a supply of usable energy?
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