Thermodynamics HW-3 (“Phase Changes & Calorimetry”): due______

Read textbook sections 12.5 & 12.6.

Conceptual Questions

1. Isopropyl alcohol is sometimes rubbed onto a patient’s arms and legs to lower their body temperature. Why is this effective?

2. As the temperature of ice is increased it changes first into a liquid and then into a vapor. On the other hand, dry ice, which is solid carbon dioxide, changes directly from a solid to a vapor as its temperature is increased. How might one produce liquid carbon dioxide?

3. A drop of water on a kitchen counter evaporates in a matter of minutes. However, only a relatively small fraction of the molecules in the drop move rapidly enough to escape through the drop’s surface. Why, then, does the entire drop evaporate rather than just a small fraction of it?

4. If you toss an ice cube into a swimming pool, is the water in the pool now at 0 °C? Explain.

Problems

Section 12.5 Latent Heat (Heat of Transformation) Refer to the Tables of Heats at the end of this document.

1. A heat transfer of is required to convert a block of ice at to water at 12 °C. What was the mass of the block of ice?

2. The graph below shows a temperature-versus-heat plot for 1.000 kg of water. (a) Calculate the heat corresponding to the points A, B, C, and D. (b) Calculate the slope of the line from point B to point C. Show that this slope is equal to 1/c, where c is the specific heat of liquid water.

Figure 17-21

3. Suppose the 1.000 kg of water in the graph above starts at point A at time zero. Heat is added to this system at the rate of 12,250 J/s. How long does it take for the system to reach (a) point B, (b) point C and (c) point D? (d) Describe the physical state of the system at time

4. When you go out to your car one cold winter morning you discover a 0.50-cm thick layer of ice on the windshield, which has an area of If the temperature of the ice is and its density is find the heat required to melt all the ice.

Section 12.6 Phase Changes and Energy Conservation

5. A large punch bowl holds 3.95 kg of lemonade (which is essentially water) at 20.0 °C. A 0.0450-kg ice cube at is placed in the lemonade. What is the final temperature of the system, and the amount of ice (if any) remaining? Ignore any heat exchange with the bowl or the surroundings.

6. An 825-g iron block is heated to 352 °C and placed in an insulated container (of negligible heat capacity) containing 40.0 g of water at 20.0 °C. What is the equilibrium temperature of this system? If your answer is 100 °C, determine the amount of water that has vaporized. The average specific heat of iron over this temperature range is560 J/(kg×K).

7. To help keep her barn warm on cold days, a farmer stores 845 kg of warm water in the barn. How many hours would a 2.00-kilowatt electric heater have to operate to provide the same amount of heat as is given off by the water as it cools from 20.0 °C to 0 °C and then freezes at 0 °C?

8. Students on a spring break picnic bring a cooler that contains 5.5 kg of ice at 0.0 °C. The cooler has walls that are 4.2 cm thick and are made of Styrofoam, which has a thermal conductivity of 0.030 W/(m×C°). The surface area of the cooler is and it rests in the shade where the air temperature is 21 °C. (a) Find the rate at which heat flows into the cooler. (b) How long does it take for the ice in the cooler to melt?

Answers

1. 2.3 kg

2. (a) QA = 4.18 x 104 J QB = 3.77 x 105 J QC = 7.96 x 105 J QD = 3.06 x 106 J (b) slope = 2.39 x 10-4 C°/J = 1/c

3. (a) 27.3s (b) 61.5 s (c) 246 s (d) boiling water

4. Q = 2.5 MJ

5. Tf = 18.8 °C

6. All the water vaporizes. Tf = 123 °C

7. t = 49.1 hours

8. (a) Q/t = 23 W (b) t = 23 hours