Situation:The specific heat of an object can be measured by placing it inthermal contact with another object whose specific heat is known.As an example, suppose that a chunk of metal, whose mass is0.37 kg, is immersed in boiling water (100 °C) until it reachesthermal equilibrium, at which time it has a temperature of 100 °C.The chunk of metal is then quickly transferred into a styrofoam (insulating) cup containing 0.3 kg of water at 20 °C. After a minute orso, the temperature of the contents of the cup stabilizes at 33 °C.Assume that once the metal is added to the cup the only energytransfer is between the hot metal and the colder water. In otherwords, there are no significant energy transfers to either the cupitself or to the surroundings.The specific heat of water in the relevant range of temperature isroughly 4.2 kJ kg1°c-1,Question:What is the specific heat of the metal?Hint:Solving this problem requires 4 steps:1) Calculate the amount of heat gained by the water.2) Use energy conservation to relate the heat gained by the waterto the heat lost by the metal. This should determine the heat lostby the metal.3) Use the bont l

Mass of chunk of metal (m)= 0.37 kg Initial temperature of chunk of metal before being placed in…

Answered: The specific heat of an object can be…

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

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A block of metal of mass 0.280 kg is heated to 148.0°C and dropped in a copper calorimeter of mass 0.250 kg that contains 0.190 kg of water at 30°C. The calorimeter and its contents are insulated from the environment and have a final temperature of 44.0°C upon reaching thermal equilibrium. Find the specific heat of the metal. Assume the specific heat of water is 4.190 x 103 J/(kg · K) and the specific heat of copper is 386 J/(kg · K). 3/(kg K)
A child running a temperature of 101°F is given an antipyrin (i.e. a medicine that lowers fever) which causes an increase in the rate of evaporation of sweat from his body. If the fever is brought down to 98 °F in 20 minutes, what is the average rate of extra evaporation caused, by the drug. Assume the evaporation mechanism to be the only way by which heat is lost. The mass of the child is 30 kg. The specific heat of human body is approximately the same as that of water, and latent heat of evaporation of water at that temperature is about 580 cal g-1.
A block of copper with a mass of 1.75 kg, initially at a temperature of 150.0°C, is in a well-insulated container. Water at a temperature of 26.0°C is added to the container, and the entire interior of the container is allowed to come to thermal equilibrium, where it reaches a final temperature of 66.0°C. What mass of water (in kg) was added? Assume any water turned to steam subsequently recondenses. ?kg
An insulated container is partly filled with oil. The lid of the container is removed, 0.150 kg of water heated to 84.0°C is poured in, and the lid is replaced. As the water and the oil reach equilibrium, the volume of the oil increases by 1.00x105 m³. The density of the oil is 919 kg/m³, its specific heat capacity is 1980 J/(kg-C°), and its coefficient of volume expansion is 726x10-6 (Cº)-¹. What is the temperature when the oil and the water reach equilibrium? Number Units
Though Babatunde's family take oats for breakfast, her mum decides that today they would take tea. She prepares it and serves Babatunde in an aluminium cup of mass 120 g. Before serving the tea, the cup had a temperature of 20 °C. The 0.30 kg tea that is poured into the cup is at a temperature of 70 °C. Determine the final temperature when thermal equilibrium is attained between the tea and the cup, assuming no exchange of heat with the surounding? (Cen is 4190 J/kg. K, cal = 910 J/kg.K).
A glass container with an insulating cover with a surface area of ( R +150)cm2 and (R+10)mm thick is filled with ice at 0 °C and placed in a second vessel maintained at a temperature of (R+ 80)°C. Find the mass of the ice that melts per minute when the flow of heat becomes steady. Specific latent heat of ice = 3.36×105J/kg and K for glass is 1W/mK. R= 83
A block of metal of mass 0.220 kg is heated to 152.0°C and dropped in a copper calorimeter of mass 0.250 kg that contains 0.200 kg of water at 30°C. The calorimeter and its contents are insulated from the environment and have a final temperature of 46.0°C upon reaching thermal equilibrium. Find the specific heat of the metal in J/(kg · K). Assume the specific heat of water is 4.190 ✕ 103 J/(kg · K) and the specific heat of copper is 386 J/(kg · K).
A copper block with a mass of 400 grams is cooled to 77 K by being immersed in liquid nitrogen. The block is then placed in a Styrofoam cup containing some water that is initially at +50.0°C. Assume no heat is transferred to the cup or the surroundings. The specific heat of liquid water is 4186 J/(kg °C), of solid water is 2060 J/(kg °C), and of copper is 385 J/(kg °C). The latent heat of fusion of water is 3.35 x 105 J/kg. What is the mass of water in the cup, if the final temperature is -25.0°C?
1. (a) How much heat transfer is necessary to raise the temperature of a 0.26 -kg piece of ice from -20 °C to 130 °C, including the 20 kJ/s energy needed for phase changes? Specific heat of ice = 2.090 kJ/kg °C Specific heat of water = 4.186 kJ/kg °C Specific heat of steam = 1.520 kJ/kg °C Heat of fusion of water = 334 kJ/kg Heat of vaporization = 2256 kJ/kg (i) Heat needed to warm ice to 0 °C: Q₁: ✔KJ (ii) Heat needed to melt ice at 0 °C: Q₂: KJ (iii) Heat required to warm 0 °C water to 100 °C: Q3: KJ (iv) Heat required to vaporize water at 100 °C: Q4: KJ (v) Heat required to warm 100 °C vapor to 130 °C: Q5: KJ Total heat, Q: KJ (b) How much time is required for the entire process, assuming a constant 20.0 kJ/s rate of heat transfer? Total time, t: S
A cube of ice is taken from the freezer at -9.5 °C and placed in a 95-g aluminum calorimeter filled with 300 g of water at room temperature of 20.0 °C. The final situation is observed to be all water at 16.0 °C. The specific heat of ice is 2100 J/kg · C°, the specific heat of aluminum is 900 J/kg · C°, the specific heat of water is is 4186 J/kg·C°, the heat of fusion of water is 333 kJ/Kg. Part A What was the mass of the ice cube? Express your answer to two significant figures and include the appropriate units. ? Value Units m = Submit Request Answer
A block of metal of mass 0.200 kg is heated to 152.0°C and dropped in a copper calorimeter of mass 0.250 kg that contains 0.150 kg of water at 30°C. The calorimeter and its contents are insulated from the environment and have a final temperature of 46.0°C upon reaching thermal equilibrium. Find the specific heat of the metal. Assume the specific heat of water is 4.190 × 103 J/(kg · K) and the specific heat of copper is 386 J/(kg · K). J/(kg · K)
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…

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