Transfer of energy

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  1. Observe an ice cube. 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?


Last Updated on October 9, 2019 by EssayPro

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