Following vigorous exercise, the internal body temperature of a 72.5-kg person is 40.0°C. At what rate, in watts, must the person transfer thermal energy to reduce the body temperature to 37.0°C in 30.0 min, assuming the body continues to produce energy at the rate of 150 W?
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Following vigorous exercise, the internal body temperature of a 72.5-kg person is 40.0°C.
At what rate, in watts, must the person transfer thermal energy to reduce the body temperature to 37.0°C in 30.0 min, assuming the body continues to produce energy at the rate of 150 W?
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- An unknown substance has a mass of 0.125 kg and an initial temperature of 94.5°C. The substance is then dropped into a calorimeter made of aluminum containing 0.285 kg of water initially at 25.5°C. The mass of the aluminum container is 0.150 kg, and the temperature of the calorimeter increases to a final equilibrium.temperature of 32.0°C. Assuming no thermal energy is transferred to the environment, calculate the specific heat of the unknown substance. J/kg - °C Need Help? Read It MY NOTES ASK YOUR TEACHER PRACTICE ANOTHER SERCP11 11.4.P.033.MI.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…During a marathon race David uses energy at a rate of 292 W. What volume of body fluid does he lose in the 5.5 hours of the race if 17.0% of the energy goes to the muscle tissue and the rest is used in removing the perspiration from the body. The latent heat of vaporization is 2.41*10^6 J/kg at 37.0°C and density of water is 1000 kg/m3. Answer in cubic meters.
- A 95.0-kg block of ice at 0.00°C breaks off from a glacier, slides along the frictionless ice to the ground from a height of 2.43 m, and then slides along a horizontal surface consisting of gravel and dirt. Find how much of the mass of the ice is melted by the friction with the rough surface, assuming 75.0% of the internal energy generated stays in the ice. Latent heat of fusion (Lf) for water 333,700 J/kg.A block of iron (c=448.00 J/kj°C) initially at temperature 6.00°C is dropped into an insulated container filled with 15.71kg of water ( cwater=4186.00 J/kg°C) at 93.00°C. They come to equilibrium at a final temperature of 39.00°C. Determine the mass of the iron block. _____kg Determine the magnitude of thermal energy Q transferred between the two substances. ______kJAn unknown substance has a mass of 0.250 kg and an initial temperature of 90.0°C. The substance is then dropped into a calorimeter made of aluminum containing 0.300 kg of water initially at 25.0°C (assume the water and calorimeter start in thermal equilibrium). The mass of the aluminum container is 0.200 kg, and the temperature of the calorimeter increases to a final equilibrium temperature of 32.0°C. Assuming no thermal energy is transferred to the environment, calculate the specific heat of the unknown substance. The specific heat of water is 4186 J/(K*mol) and aluminum is 900 J/(K*mol).
- A 155 g copper bowl contains 230 g of water, both at 20.0°C. A very hot 300 g copper cylinder is dropped into the water, causing the water to boil, with 4.05 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy (in calories) is transferred to the water as heat? 8.6 X kcal (b) How much energy (in calories) is transferred to the bowl? 55 X kcal (c) What is the original temperature of the cylinder? 553.6 X °C Did you use the idea of conservation of energy? That is, did you equate the sum of the energy transfers to zero? For the bowl and cylinder, did you substitute the expression relating an energy transfer, the specific heat, the mass, and the temperature change? For the water, did you use the same expression to get the water to the boiling point? Did you also include an expression for the heat of vaporization? Did you use the given final temperature for each of the three materials?Large meteors sometimes strike the Earth, converting most of their kinetic energy into thermal energy. (a) What is the kinetic energy of a 109kg meteor moving at 25.0 km/s? (b) If this meteor lands in a deep ocean and 80% of its kinetic energy goes into heating water, how many kilograms of water could it raise by 5.0°C?A 0.100 kg piece of ice at initial temperature −5.00 ◦C is placed in a perfectly insulated container with 1.00 kg (1 L) of water at initial temperature 20.0 ◦C. The container absorbs or releases no heat. All of the ice melts as the system reaches an equilibrium temperature Tf . How much heat must the ice exchange with the rest of the system to raise its temperature to the melting point, 0.00 ◦C? Would this heat exchanged be positive, zero, or negative? Once the ice reaches its melting point, how much heat must the ice exchange with the rest of the system to melt? Would this heat exchanged be positive, zero, or negative? Once the ice melts, it is liquid water at 0.00 ◦C. Write an expression for the heat exchanged by the newly-melted ice QI to reach the equilibrium temperature Tf . Would you expect QI to be positive, zero, or negative? Write an expression for the heat exchanged by the original water QW to reach the equilibrium temperature Tf from its initial temperature. Assuming no…