Chapter 18: Problem 17
Why does tile feel so much colder to your feet after a bath than a bath rug? Why is this effect more striking when your feet are cold?
Chapter 18: Problem 17
Why does tile feel so much colder to your feet after a bath than a bath rug? Why is this effect more striking when your feet are cold?
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Get started for freeEnhanced geothermal systems (EGS) consist of two or more boreholes that extend several kilometers below ground level into the hot bedrock. Since drilling these holes can cost millions, one concern is that the heat provided by the bedrock cannot pay back the initial investment. Suppose \(0.493 \mathrm{~km}^{3}\) of granite is to be drawn on for \(124.9 \mathrm{yr}\) and in the process will cool from \(169.9^{\circ} \mathrm{C}\) to \(105.5^{\circ} \mathrm{C} .\) What is the average power the granite can deliver during that time? [The density of granite is 2.75 times that of water, and its specific heat is \(\left.0.790 \mathrm{~kJ} /\left(\mathrm{kg}^{\circ} \mathrm{C}\right) .\right]\)
In one of your rigorous workout sessions, you lost \(150 . \mathrm{g}\) of water through evaporation. Assume that the amount of work done by your body was \(1.80 \cdot 10^{5} \mathrm{~J}\) and that the heat required to evaporate the water came from your body. a) Find the loss in internal energy of your body, assuming that the latent heat of vaporization is \(2.42 \cdot 10^{6} \mathrm{~J} / \mathrm{kg} .\) b) Determine the minimum number of food calories that must be consumed to replace the internal energy lost ( 1 food calorie \(=4186 \mathrm{~J}\) ).
For a class demonstration, your physics instructor pours \(1.00 \mathrm{~kg}\) of steam at \(100.0^{\circ} \mathrm{C}\) over \(4.00 \mathrm{~kg}\) of ice at \(0.00^{\circ} \mathrm{C}\) and waits for the system to reach equilibrium, when he will measure the temperature. While the system reaches equilibrium, you are given the latent heats of ice and steam and the specific heat of water: \(L_{\text {ice }}=3.33 \cdot 10^{5} \mathrm{~J} / \mathrm{kg}, L_{\text {steam }}=2.26 \cdot 10^{6} \mathrm{~J} / \mathrm{kg}\), \(c_{\text {water }}=4186 \mathrm{~J} /\left(\mathrm{kg}^{\circ} \mathrm{C}\right) .\) You are asked to calculate the final equilibrium temperature of the system. What value do you find?
A material has mass density \(\rho\), volume \(V\), and specific heat \(c\). Which of the following is a correct expression for the heat exchange that occurs when the material's temperature changes by \(\Delta T\) in degrees Celsius? a) \((\rho c / V) \Delta T\) b) \((\rho c V)(\Delta T+273.15)\) c) \((\rho c V) / \Delta T\) d) \(\rho c V \Delta T\)
How much thermal energy is needed to melt a 3.0 -kg copper block that is initially at a temperature of \(1359 \mathrm{~K} ?\) a) \(101 \mathrm{~kJ}\) b) \(221 \mathrm{~kJ}\) c) \(390 \mathrm{~kJ}\) d) \(615 \mathrm{~kJ}\) e) \(792 \mathrm{~kJ}\)
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