A system undergoes a two-step process. In the first step, the internal energy of the system increases by 229 J when 166 J of work is done on the system. In the second step, the internal energy of the system increases by 115 J when 169 J of work is done on the system. For the overall process, fine the heat added to the system (including sign).
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- 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).In a game of football outdoors on a cold day, a player will begin to feel exhausted after using approximately 8.0 x 10 J of internal energy. (a) One player, dressed too lightly for the weather, has to leave the game after losing 7.0 x 10° Jof heat. How much work has he done? (b) Another player, wearing clothes that offer better protection against heat loss, is able to remain in the game long enough to do 2.3x 105 J of work. What is the magnitude of the heat that he has lost? (a) Number Units (b) Number Units <.A system undergoes a two-step process. In the first step, the internal energy of the system increases by 230 J when 166 J of work is done on the system. In the second step, the internal energy of the system increases by 115 J when 191 J of work is done on the system. For the overall process, find the heat added to the system (including sign).
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- Three moles of an ideal monatomic gas are at a temperature of 383 K. Then 2892 J of heat is added to the gas, and 714 J of work is done on it. What is the final temperature of the gas?A gas at 0.75 atm with a volume of 21.7 L undergoes a quasi-static isobaric expansion. If during this process the gas does 457 J of work and its internal energy increases by 73 J, how much heat does the gas absorb?A closed gas system has 682 J of heat gain from the environment and 439 J of work is done on the gas causing it to be compressed. Calculate the change in internal energy of the gas.
- What is the change in internal energy of a system which does 0.42 J of work while 8.87 J of heat transfer occurs into the system, and 8.87 J of heat transfer occurs to the environment? Give your answer in joules.The water in a deep underground well is used as the cold resevoir of a Carnot heat pump that maintains the temperature of a house at 303 K. To deposit 13000 J of heat in the house, the heat pump requires 716 J of work. Determine the temperature of the well water.What is the change in internal energy of a system that takes in 4.53 x 106 ) of heat, and does 4.50 x 105 J of work while dissipating 8.67 x 106 J of heat?