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Chapter 19: Q. 6 (page 543)
a. Is the final temperature higher than, lower than, or equal to the initial temperature?
b. Is any heat energy added to or removed from the system in this process? Explain
a. The final temperature is greater than initial temperature.
b. No heat exchange has ben seen in the system.
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Draw a first-law bar chart (see Figure 19.12) for the gas process in Figure EX19.6.
The burner on an electric stove has a power output of 2.0 kW. A 750 g stainless steel teakettle is filled with 20°C water and placed on the already hot burner. If it takes 3.0 min for the water to reach a boil, what volume of water, in cm3, was in the kettle? Stainless steel is mostly iron, so you can assume its specific heat is that of iron.
An experiment measures the temperature of a 500 g substance
while steadily supplying heat to it. Figure EX19.20 shows the
results of the experiment. What are the (a) specific heat of the
solid phase, (b) specific heat of the liquid phase, (c) melting and
boiling temperatures, and (d) heats of fusion and vaporization?
of gas are at and a pressure of . How much work must be done on the gas to compress it to one-third of its initial volume at (a) constant temperature and (b) constant pressure? (c) Show both processes on a singlediagram.
When air is inhaled, it quickly becomes saturated with water vapor as it passes through the moist airways. Consequently, an adult human exhales about 25 mg of evaporated water with each breath. Evaporation—a phase change—requires heat, and the heat energy is removed from your body. Evaporation is much like boiling, only water’s heat of vaporization at 35°C is a somewhat larger 24 * 105 J/kg because at lower temperatures more energy is required to break the molecular bonds. At 12 breaths/min, on a dry day when the inhaled air has almost no water content, what is the body’s rate of energy loss (in J/s) due to exhaled water? (For comparison, the energy loss from radiation, usually the largest loss on a cool day, is about 100 J/s.)
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