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1.1. The actual amount (mass) of gasoline left in the tank when the gauge hits “empty” is less in the summer than in the winter. The gasoline has the same volume as it does in the winter when the “add fuel” light goes on, but because the gasoline has expanded, there is less mass.

1.2. Not necessarily, as the thermal stress is also proportional to Young’s modulus.

1.3. To a good approximation, the heat transfer depends only on the temperature difference. Since the temperature differences are the same in both cases, the same 25 kJ is necessary in the second case. (As we will see in the next section, the answer would have been different if the object had been made of some substance that changes phase anywhere between 30°C and 50°C.)

1.4. The ice and liquid water are in thermal equilibrium, so that the temperature stays at the freezing temperature as long as ice remains in the liquid. (Once all of the ice melts, the water temperature will start to rise.)

1.5. Snow is formed from ice crystals and thus is the solid phase of water. Because enormous heat is necessary for phase changes, it takes a certain amount of time for this heat to be transferred from the air, even if the air is above 0°C.

1.6. Conduction: Heat transfers into your hands as you hold a hot cup of coffee. Convection: Heat transfers as the barista “steams” cold milk to make hot cocoa. Radiation: Heat transfers from the Sun to a jar of water with tea leaves in it to make “Sun tea.” A great many other answers are possible.

1.7. Because area is the product of two spatial dimensions, it increases by a factor of four when each dimension is doubled ($$\displaystyle A_{final}=(2d)^2=4d^2=4A_{initial}$$). The distance, however, simply doubles. Because the temperature difference and the coefficient of thermal conductivity are independent of the spatial dimensions, the rate of heat transfer by conduction increases by a factor of four divided by two, or two: $$\displaystyle P_{final}=\frac{kA_{final}(T_h−T_c)}{d_{final}}=\frac{k(4A_{final}(T_h−T_c))}{2d_{initial}}=2\frac{kA_{final}(T_h−T_c)}{d_{initial}}=2P_{initial}$$.

1.8. Using a fan increases the flow of air: Warm air near your body is replaced by cooler air from elsewhere. Convection increases the rate of heat transfer so that moving air “feels” cooler than still air.

1.9. The radiated heat is proportional to the fourth power of the absolute temperature. Because $$\displaystyle T_1=293K$$ and $$\displaystyle T_2=313K$$, the rate of heat transfer increases by about 30% of the original rate.

Conceptual Questions

1. They are at the same temperature, and if they are placed in contact, no net heat flows between them.

5. The cold water cools part of the inner surface, making it contract, while the rest remains expanded. The strain is too great for the strength of the material. Pyrex contracts less, so it experiences less strain.

7. In principle, the lid expands more than the jar because metals have higher coefficients of expansion than glass. That should make unscrewing the lid easier. (In practice, getting the lid and jar wet may make gripping them more difficult.)

9. After being heated, the length is $$\displaystyle (1+300α)(1m)$$. After being cooled, the length is $$\displaystyle (1−300α)(1+300α)(1m)$$. That answer is not 1 m, but it should be. The explanation is that even if $$\displaystyle α$$ is exactly constant, the relation $$\displaystyle ΔL=αLΔT$$ is strictly true only in the limit of small $$\displaystyle ΔT$$. Since $$\displaystyle α$$ values are small, the discrepancy is unimportant in practice.

11. Temperature differences cause heat transfer.

13. No, it is stored as thermal energy. A thermodynamic system does not have a well-defined quantity of heat.

15. It raises the boiling point, so the water, which the food gains heat from, is at a higher temperature.

17. Yes, by raising the pressure above 56 atm.

19. work

21. 0°C (at or near atmospheric pressure)

23. Condensation releases heat, so it speeds up the melting.

25. Because of water’s high specific heat, it changes temperature less than land. Also, evaporation reduces temperature rises. The air tends to stay close to equilibrium with the water, so its temperature does not change much where there’s a lot of water around, as in San Francisco but not Sacramento.

27. The liquid is oxygen, whose boiling point is above that of nitrogen but whose melting point is below the boiling point of liquid nitrogen. The crystals that sublime are carbon dioxide, which has no liquid phase at atmospheric pressure. The crystals that melt are water, whose melting point is above carbon dioxide’s sublimation point. The water came from the instructor’s breath.

29. Increasing circulation to the surface will warm the person, as the temperature of the water is warmer than human body temperature. Sweating will cause no evaporative cooling under water or in the humid air immediately above the tub.

31. It spread the heat over the area above the heating elements, evening the temperature there, but does not spread the heat much beyond the heating elements.

33. Heat is conducted from the fire through the fire box to the circulating air and then convected by the air into the room (forced convection).

35. The tent is heated by the Sun and transfers heat to you by all three processes, especially radiation.

37. If shielded, it measures the air temperature. If not, it measures the combined effect of air temperature and net radiative heat gain from the Sun.

39. Turn the thermostat down. To have the house at the normal temperature, the heating system must replace all the heat that was lost. For all three mechanisms of heat transfer, the greater the temperature difference between inside and outside, the more heat is lost and must be replaced. So the house should be at the lowest temperature that does not allow freezing damage.

41. Air is a good insulator, so there is little conduction, and the heated air rises, so there is little convection downward.

Problems

43. That must be Celsius. Your Fahrenheit temperature is 102°F. Yes, it is time to get treatment.

45. a. $$\displaystyle ΔT_C=22.2°C$$;

b. We know that $$\displaystyle ΔT_F=T_{F2}−T_{F1}$$. We also know that $$\displaystyle T_{F2}=\frac{9}{5}T_{C2}+32$$ and $$\displaystyle T_{F1}=\frac{9}{5}T_{C1}+32$$. So, substituting, we have $$\displaystyle ΔT_F=(\frac{9}{5}T_{C2}+32)−(\frac{9}{5}T_{C1}+32)$$. Partially solving and rearranging the equation, we have $$\displaystyle ΔT_F=\frac{9}{5}(T_{C2}−T_{C1})$$. Therefore, $$\displaystyle ΔT_F=\frac{9}{5}ΔT_C$$ΔTF=95ΔTC.

47. a. −40°; b. 575 K

49. Using Table 1.2 to find the coefficient of thermal expansion of marble:

$$\displaystyle L=L_0+ΔL=L_0(1+αΔT)=170m[1+(2.5×10^{−6}/°C)(−45.0°C)]=169.98m$$

(Answer rounded to five significant figures to show the slight difference in height.)

51. We use $$\beta$$ instead of $$\alpha$$ since this is a volume expansion with constant surface area. Therefore:

$$\displaystyle ΔL=αLΔT=(6.0×10^{−5}/°C)(0.0300m)(3.00°C)=5.4×10^{−6}m$$.

53. On the warmer day, our tape measure will expand linearly. Therefore, each measured dimension will be smaller than the actual dimension of the land. Calling these measured dimensions l'l' and w'w', we will find a new area, A. Let’s calculate these measured dimensions:

$$\displaystyle l'=l_0−Δl=(20m)−(20°C)(20m)(\frac{1.2×10^{−5}}{°C})=19.9952m$$

$$\displaystyle A'=l×w'=(29.9928m)(19.9952m)=599.71m^2$$

Cost change = $$\displaystyle (A−A')(\frac{60,000}{m^2})=((600−599.71)m^2)(\frac{60,000}{m^2})=17,000$$

Because the area gets smaller, the price of the land decreases by about $17,000. 55. a. Use Table 1.2 to find the coefficients of thermal expansion of steel and aluminum. Then $$\displaystyle ΔL_{Al}−ΔL_{steel}=(α_{Al}−α_{steel})L_0ΔT=(\frac{2.5×10^{−5}}{°C}−\frac{1.2×10^{−5}}{°C})(1.00m)(22°C)=2.9×10^{−4}m$$ b. By the same method with $$\displaystyle L_0=30.0m$$, we have $$\displaystyle ΔL=8.6×10^{−3}m$$. 57. $$\displaystyle ΔV=0.475L$$ 59. If we start with the freezing of water, then it would expand to $$\displaystyle (1m^3)(\frac{1000kg/m^3}{917kg/m^3})=1.09m^3=1.98×10^8N/m^2$$ of ice. 61. $$\displaystyle m=5.20×10^8J$$ 63. $$\displaystyle Q=mcΔT⇒ΔT=\frac{Q}{mc}$$; a. 21.0°C; b. 25.0°C; c. 29.3°C; d. 50.0°C 65. $$\displaystyle Q=mcΔT⇒c=\frac{Q}{mΔT}=\frac{1.04kcal}{(0.250kg)(45.0°C)}=0.0924kcal/kg⋅°C$$. It is copper. 67. a. $$\displaystyle Q=m_wc_wΔT+m_{A1}c_{A1}ΔT=(m_wc_w+m_{A1}c_{A1})ΔT; \(\displaystyle Q=[(0.500kg)(1.00kcal/kg⋅°C)+(0.100kg)(0.215kcal/kg⋅°C)](54.9°C)=28.63kcal$$; $$\displaystyle \frac{Q}{m_p}=\frac{28.63kcal}{5.00g}=5.73kcal/g;$$ b. $$\displaystyle \frac{Q}{m_p}=\frac{200kcal}{33g}=6kcal/g$$, which is consistent with our results to part (a), to one significant figure. 69. 0.139°C 71. It should be lower. The beaker will not make much difference: 16.3°C 73. a. $$\displaystyle 1.00×10^5J$$; b. $$\displaystyle 3.68×10^5J$$; c. The ice is much more effective in absorbing heat because it first must be melted, which requires a lot of energy, and then it gains the same amount of heat as the bag that started with water. The first $$\displaystyle 2.67×10^5J$$ of heat is used to melt the ice, then it absorbs the $$\displaystyle 1.00×10^5J$$ of heat as water. 75. 58.1 g 77. Let M be the mass of pool water and m be the mass of pool water that evaporates. $$\displaystyle McΔT=mLV_{(37°C)}⇒\frac{m}{M}=\frac{cΔT}{L_{V(37°C)}}=\frac{(1.00kcal/kg⋅°C)(1.50°C)}{580kcal/kg}=2.59×10^{−3}$$; (Note that $$\displaystyle L_V$$ for water at 37°C is used here as a better approximation than $$\displaystyle L_V$$ for 100°C water.) 79. a. $$\displaystyle 1.47×10^{15}kg$$; b. $$\displaystyle 4.90×10^{20}J$$; c. $$\displaystyle 48.5 y$$ 81. a. 9.35 L; b. Crude oil is less dense than water, so it floats on top of the water, thereby exposing it to the oxygen in the air, which it uses to burn. Also, if the water is under the oil, it is less able to absorb the heat generated by the oil. 83. a. 319 kcal; b. 2.00°C 85. First bring the ice up to 0°C and melt it with heat $$\displaystyle Q_1$$: 4.74 kcal. This lowers the temperature of water by $$\displaystyle ΔT_2: 23.15°C$$. Now, the heat lost by the hot water equals that gained by the cold water ($$\displaystyle T_f$$ is the final temperature): 20.6°C 87. Let the subscripts r, e, v, and w represent rock, equilibrium, vapor, and water, respectively. $$\displaystyle m_rc_r(T_1−T_e)=m_VL_V+m_Wc_W(T_e−T_2)$$; $$\displaystyle m_r=\frac{m_VL_V+m_Wc_W(T_e−T_2)}{c_r(T_1−T_e)}=\frac{(0.0250kg)(2256×10^3J/kg)+(3.975kg)(4186×10^3J/kg⋅°C)(100°C−15°C)}{(840J/kg⋅°C)(500°C−100°C)}=4.38kg$$ 89. a. $$\displaystyle 1.01×10^3W$$; b. One 1-kilowatt room heater is needed. 91. 84.0 W 93. 2.59 kg 95. a. 39.7 W; b. 820 kcal 97. $$\displaystyle \frac{Q}{t}=\frac{kA(T_2−T_1)}{d}, so that \frac{(Q/t)_{wall}}{(Q/t)_{window}}=\frac{k_{wall}A_{wall}d_{window}}{k_{window}A_{window}d_{wall}}=\frac{(2×0.042J/s⋅m⋅°C)(10.0m^2)(0.750×10^{−2}m)}{(0.84J/s⋅m⋅°C)(2.00m^2)(13.0×10^{−2}m)}$$ This gives 0.0288 wall: window, or 35:1 window: wall 99. $$\displaystyle \frac{Q}{t}=\frac{kA(T_2−T_1)}{d}=\frac{kAΔT}{d}⇒ΔT=\frac{d(Q/t)}{kA}=\frac{(6.00×10^{−3}m)(2256W)}{(0.84J/s⋅m⋅°C)(1.54×10^{−2}m^2)}=1046°C=1.05×10^3K$$ 101. We found in the preceding problem that $$\displaystyle P=126ΔTW⋅°C$$ as baseline energy use. So the total heat loss during this period is $$\displaystyle Q=(126J/s⋅°C)(15.0°C)(120days)(86.4×10^3s/day)=1960×10^6J$$. At the cost of$1/MJ, the cost is $1960. From an earlier problem, the savings is 12% or$235/y. We need $$\displaystyle 150m^2$$ of insulation in the attic. At $$\displaystyle 4/m^2$$, this is a \$500 cost. So the payback period is $$\displaystyle 600/(235/y)=2.6years$$ (excluding labor costs).

103. 7.39%

105. $$\displaystyle \frac{F}{A}=(210×10^9Pa)(12×10^{−6}/°C)(40°C−(−15°C))=1.4×10^8N/m^2$$

107. a. 1.06 cm;

b. 1.11 cm

109. $$\displaystyle 1.7kJ/(kg⋅ºC)$$

111. a. $$\displaystyle 1.57×10^4kcal$$;

b. $$\displaystyle 18.3kW⋅h$$;

c. $$\displaystyle 1.29×10^4$$ kcal

113. 6.3°C. All of the ice melted.

115. 63.9°C, all the ice melted

117. a. 83 W;

b. $$\displaystyle 1.97×10^3W$$; The single-pane window has a rate of heat conduction equal to 1969/83, or 24 times that of a double-pane window.

119. The rate of heat transfer by conduction is 20.0 W. On a daily basis, this is 1,728 kJ/day. Daily food intake is 2400kcal/d×4186J/kcal=10,050kJ/day. So only 17.2% of energy intake goes as heat transfer by conduction to the environment at this $$\displaystyle ΔT$$.

121. 620 K

Challenge Problems

123. Denoting the period by P, we know $$\displaystyle P=2π\sqrt{L/g}$$. When the temperature increases by dT, the length increases by $$\displaystyle αLdT$$. Then the new length is a. $$\displaystyle P=2π\sqrt{L+αLdT}{g}=2π\sqrt{\frac{L}{g}(1+αdT)}=2π\sqrt{\frac{L}{g}}(1+\frac{1}{2}αdT)=P(1+\frac{1}{2}αdT)$$ by the binomial expansion. b. The clock runs slower, as its new period is 1.00019 s. It loses 16.4 s per day.

125. The amount of heat to melt the ice and raise it to 100°C is not enough to condense the steam, but it is more than enough to lower the steam’s temperature by 50°C, so the final state will consist of steam and liquid water in equilibrium, and the final temperature is 100°C; 9.5 g of steam condenses, so the final state contains 49.5 g of steam and 40.5 g of liquid water.

127. a. $$\displaystyle dL/dT=kT/ρL$$;

b. $$\displaystyle L=\sqrt{2kTt/ρL_f}$$;

c. yes

129. a. $$\displaystyle σ(πR^2)T_s^4$$;

b. $$\displaystyle eσπR^2T_s^4$$;

c. $$\displaystyle 2eσπR^2T_e^4$$;

d. $$\displaystyle T^4_s=2T^4_eT_s^4=2T_e^4$$;

e. $$\displaystyle eσT^4_s+\frac{1}{4}(1−A)S=σT^4_s$$;

f. 288 K