A class of 10 students taking an exam has a power output per student of about 200 W. Assume the initial temperature of the room is 20°C and that its dimensions are 6.0 m by 15.0 m by 3.0 m. What is the temperature of the room at the end of 1.0 h if all the energy remains in the air in the room and none is added by an outside source? The specific heat of air is 837 J/kg · °C, and its density is about 1.3 x 10–3 g/cm3.
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![A class of 10 students taking an exam has a
power output per student of about 200 W.
Assume the initial temperature of the room
is 20°C and that its dimensions are 6.0 m by
15.0 m by 3.0 m. What is the temperature of
the room at the end of 1.0 h if all the energy
remains in the air in the room and none is
added by an outside source? The specific
heat of air is 837 J/kg · °C, and its density is
about 1.3 × 10-3 g/cm3.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbee2a0c0-a619-418d-86bc-762868c24935%2Ff262e622-cba7-4ca4-90a0-5f4985aa3a2e%2F2v47pud_processed.jpeg&w=3840&q=75)
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- A solid sphere has a temperature of 603 K. The sphere is melted down and recast into a cube that has the same emissivity and emits the same radiant power as the sphere. What is the cube's temperature in kelvins?Imagine a physics lecture hall with 83 students who are settling in for a 1-hour lecture. At the start of the lecture, the temperature of the air in the room is a comfortable 70oF (21.1°C). Unfortunately, the room’s air conditioner breaks right as the lecture begins. Each student has an average power output of about 60.0 W at room temperature. Imagine the energy released by each student goes into heating just the air in the room, which has a volume of 9.50 × 102 m3 and a density of 1.20 kg/m3. Assume the volume of the air remains constant and the specific heat capacity of the air is 718 J/(kg · °C). Calculate the room’s temperature at the end of the lecture in oF (the answer may sound high (!), but in reality, a significant portion of the heat produced would be absorbed by the walls, ceiling, floors, chairs, desks, and so on, which we are neglecting).Part 2: Problem Solving Questions P 1 (thermodynamics). What energy is required to convert a 3.00 g cube of ice at 213.15 K to liquid water at 355.15 K ?. (constants: specific heat for ice is 2090.0 J/kg⋅°C, latent heat of fusion of ice is 3.33⋅105 J/kg, specific heat for water is 4186.0 J/kg⋅°C).
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- Rubbing your hands together warms them by converting work into thermal energy. a. If a woman rubs her hands a total of 19 times (forward and backwards count separately), at a distance of 7.75 cm per rub, and with an average frictional force of 39 N, what is the temperature increase of her hands, in degrees Celsius? The mass of tissues warmed is only 0.100 kg, mostly in the palms and fingers, and the heat capacity of her hands is 3500 J/(kg⋅°C).A chunk of hot iron is pulled out of a fire and placed between aluminum vice grips. The mass of the iron is 219 g and the mass of the aluminum is 66.4 g. The iron is initially 351.8 °C. The aluminum is initially 24.7 °C. Assuming no loss of heat to the environment, what is the final temperature of the iron-aluminum system? I couldn't even get started on this one.The electric output of a power plant is 800 MW. Cooling water flows through the power plant at the rate 1.00 x 108 L/hr. The cooling water enters the plant at 11.0 °C and exits at 29.0 °C. What is the power plant's thermal efficiency? Express your answer as a percentage.
- An unknown substance has a mass of 0.125 kg and an initial temperature of 90.0°C. The substance is then dropped into a calorimeter made of aluminum containing 0.285 kg of water initially at 21.5°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.Suppose you want to raise the temperature of a 0.18-kg piece of ice from -20.0°C to 130°C. The heat of fusion is Lf = 334 kJ/kg, and the heat of vaporization is Lv = 2256 kJ/kg. In this problem, take 1520 J/kg⋅°C as the specific heat of steam, and 2090 J/kg⋅°C as the specific heat of ice. a.) How much heat, in kilocalories, must be transferred for this to happen, including the energy needed for phase changes? b.) How much time, in seconds, is required to do this, assuming a constant 20.0 kJ/s rate of heat transfer?A 25,000 kg subway train initially traveling at 15.5 m/s slows to a stop in a station and the stays there long enoughfor its brakes to cool. The station's dimensions are 65.0 m long by 20.0 m wide by 12.0 m high. Assuming all the work done by the brakes in stopping the train is transferred as heat uniformly to all the air in the station, by how much does the air temperature in the sation rise? Take the density of the air to be 1.20 kg/m3 and its specific heat to be 1020 J/kg*K.