7.3.2.P6
A 200 g block of copper at a temperature of 55oC is put into an insulated beaker containing 200 g water at 20oC. The specific heat of water is about 1.0 J/g-oC while the specific heat of copper is only about 0.4 J/g-oC. As a result, the two come to thermal equilibrium at a temperature of about 30 oC – much closer to the original temperature of the water than of the copper.
1. From this you can conclude:
- There are more degrees of freedom in 200 g of copper than in 200 g of water.
- There are fewer degrees of freedom in 200 g of copper than in 200 g of water.
- There are about the same number of degrees of freedom in 200 g of copper as there are in 200 g of water.
- The information given doesn't tell you anything about the number of degrees of freedom in the matter.
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2. From this you can conclude that after the system has come to thermal equilibrium (choose all that apply):
- The average kinetic energy of one molecule of water is greater than that of one copper atom.
- The average kinetic energy of one molecule of water is less than that of one copper atom.
- The average kinetic energy of one molecule of water is the same as that of one copper atom.
- The information given doesn't tell you anything about the kinetic energy of the molecules/atoms.
3. Complete each sentence with I (increases), S (stays the same), D (decreases), or N (you can’t tell)
- As the copper cools off, its entropy ___
- As the water warms up, its entropy ___
- As the two substances in the isolated water-copper system come into thermal equilibrium, their total entropy ___
4. Select statements that correctly describe how the energy of the copper block behaves during the process.
- The internal energy of the copper block decreases until it reached thermal equilibrium, and then stops changing.
- The internal energy of the copper block fluctuates until it reaches thermal equilibrium, when the fluctuations stop.
- The internal energy of the copper block fluctuates throughout the experiment.
- The internal energy of the copper block did not change in the course of the experiment.
5/3/18 Bill Dorland & Joe Redish
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