(a) At what rate is his excess thermal energy dissipated by radiation? (Enter your answer to at least one decimal place.) W (b) If he eliminates 0.44 kg of perspiration during that hour, at what rate is thermal energy dissipated by evaporation of sweat? (Enter your answer to at least one decimal place.) W (c) At what rate is energy eliminated by evaporation from the lungs? (Enter your answer to at least one decimal place.) W

(a) At what rate is his excess thermal energy dissipated by radiation? (Enter your answer to at least one decimal place.) W (b) If he eliminates 0.44 kg of perspiration during that hour, at what rate is thermal energy dissipated by evaporation of sweat? (Enter your answer to at least one decimal place.) W (c) At what rate is energy eliminated by evaporation from the lungs? (Enter your answer to at least one decimal place.) W

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A block of 10.0 kg of solid gold at its melting point of 1,063.00°C changes phase to liquid gold at 1,063.00°C and then changes phase back to solid gold at 1,063.00°C. The latent heat of fusion for gold is 6.44×104 J/kg. What is the total change in internal energy of the gold during this whole process?
When energy shortages occur, magazine articles sometimes urge us to keep our homes at a constant temperature day and night to conserve fuel. They argue that when we turn down the heat at night, the walls, ceilings, and other areas cool off and must be reheated in the morning. So if we keep the temperature constant, these parts of the house will not cool off and will not have to be reheated. Does this argument make sense? Would we really save energy by following this advice?
An artist working on a piece of metal in his forging studio plunges the hot metal into oil in order to harden it. The metal piece has a mass of 62 kg and its specific heat is 0.1027 kcal/(kg · °C). He uses 810 kg of oil at 35°C. The specific heat of oil is 0.7167 kcal/(kg · °C). Once the metal is immersed in the oil, the temperature reaches an equilibrium value of 38°C. How hot was the forged metal piece just before he plunged it into the oil?
We have 39.5 g of a particular substance. Its specific heat in solid form is 0.8 J/(g K) and its specific heat in liquid form is 1.4 J/(g K); it's latent heat of melting is 170 J/g. Its initial temperature is 196 and its melting point is 223. We wish to raise its temperature to 297 (where it is a liquid). How much heat is required?
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The rate at which a resting person converts food energy is called one’s basal metabolic rate (BMR). Assume that the resulting internal energy leaves a person’s body by radiation and convection of dry air. When you jog, most of the food energy you burn above your BMR becomes internalenergy that would raise your body temperature if it were not eliminated. Assume that evaporation of perspiration is the mechanism for eliminating this energy. Suppose a person is jogging for “maximum fat burning,” converting food energy at the rate 400 kcal/h above his BMR, and putting out energy by work at the rate 60.0 W. Assume that the heat of evaporation of water at body temperature is equal to its heat of vaporization at 100°C. (a) Determine the hourly rate at which water must evaporate from his skin. (b) When you metabolize fat, the hydrogen atoms in the fat molecule are transferred to oxygen to form water. Assume that metabolism of 1.00 g of fat generates 9.00 kcal of energy and produces 1.00 g of…