A 100 g copper bowl contains 170 g of water, both at 21.0°C. A very hot 400 g copper cylinder is dropped into the water, causing the water to boil, with 16.5 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy is transferred to the water as heat? (b) How much to the bowl? (c) What is the original temperature of the cylinder? The specific heat of water is 1 cal/g. K, and of copper is 0.0923 cal/g.K. The latent heat of vaporization of water is 539 Cal/kg.

A 100 g copper bowl contains 170 g of water, both at 21.0°C. A very hot 400 g copper cylinder is dropped into the water, causing the water to boil, with 16.5 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy is transferred to the water as heat? (b) How much to the bowl? (c) What is the original temperature of the cylinder? The specific heat of water is 1 cal/g. K, and of copper is 0.0923 cal/g.K. The latent heat of vaporization of water is 539 Cal/kg.

Physics for Scientists and Engineers, Technology Update (No access codes included)

9th Edition

ISBN:9781305116399

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter20: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 20.10OQ: A 100-g piece of copper, initially at 95.0C, is dropped into 200 g of water contained in a 280-g...

See similar textbooks

Similar questions

A 100-g piece of copper, initially at 95.0C, is dropped into 200 g of water contained in a 280-g aluminum can; the water and can are initially at 15.0C. What is the final temperature of the system? (Specific heats of copper and aluminum are 0.092 and 0.215 cal/g C. respectively.) (a) 16C (b) 18C (c) 24C (d) 26C (e) none of those answers
One of a dilute diatomic gas occupying a volume of 10.00 L expands against a constant pressure of 2.000 atm when it is slowly heated. If the temperature of the gas rises by 10.00 K and 400.0 J of heat are added in the process, what is its final volume?
How much energy transfer as heat is required to evaporate completely 1 kg of nitrogen for a constant pressure process, with ? = 89.5 K?
How much energy (in Joules) is needed to be removed to freeze water, completely, so that all the water is now ice, m = 405 g, if the water has an initial temperature of 55oF? Round to 4 significant figures. cice = 2090 J/(kg oC) cwater = 4186 J/(kg oC) Lwater = 3.33 x 105 J/kg
One ton of liquid water at 80C is brought into awell-insulated and well-sealed 4-m * 5-m * 7-m room initiallyat 22C and 100 kPa. Assuming constant specific heatsfor both air and water at room temperature, determine (a) thefinal equilibrium temperature in the room and (b) the totalentropy change during this process, in kJ/K.
Assume Lake Huron contains 3.60 ✕ 1012 m3 of water, and assume the water's density is that of water at 20°C and 1 atm. (a) How much energy (in J) is required to raise the temperature of that volume of water from 12.2°C to 25.0°C? J (b) How many years would it take to supply this amount of energy by using a power of 1,200 MW generated by an electric power plant? yr
How much thermal energy must be added to 3.00 moles of monatomic ideal gas tat 300 K kept at constant volume of 1.5 L in order to raise the temperature to 400 K ?
A 0.617 mol sample of Xe(g) initially at 298 K and 1.00 atm is held at constant volume while enough heat is applied to raise the temperature of the gas by 14.9 K. Assuming ideal gas behavior, calculate the amount of heat (?)in joules required to affect this temperature change and the total change in internal energy, Δ?. Note that some books use Δ? as the symbol for internal energy instead of Δ?. Type of gas Molar heat capacity at constant volume (??,?) atoms (3/2)? linear molecules (5/2)? nonlinear molecules 3? where ? is the ideal gas constant
A 2.5 kg lump of aluminum is heated to 96oC and then dropped into 9.0 kg of water at 5.1oC. Assuming that the lump–water system is thermally isolated, what is the system's equilibrium temperature? Assume the specific heats of water and aluminum are 4186 and 900 J/kg-K, respectively.
A certain gas at a temperature equivalent to 24°C in a 9 m³ is compressed to 150 kPa to 2 m³, what is the resulting pressure in isothermal condition?
A 50-m-long section of a steam pipe whose outer diameteris 10 cm passes through an open space at 15°C. The averagetemperature of the outer surface of the pipe is measured to be150°C. If the combined heat transfer coefficient on the outer surfaceof the pipe is 20 W/m2·K, determine (a) the rate of heat lossfrom the steam pipe; (b) the annual cost of this energy lost if steamis generated in a natural gas furnace that has an efficiency of 75percent and the price of natural gas is $0.52/therm (1 therm =105,500 kJ); and (c) the thickness of fiberglass insulation(k = 0.035 W/m·K) needed in order to save 90 percent of the heatlost. Assume the pipe temperature to remain constant at 150°C.
A test is conducted to determine the overall heat transfer coefficient in anautomotive radiator that is a compact cross-flow water-to-air heat exchangerwith both fluids (air and water) unmixed. The radiator has 40 tubesof internal diameter 0.5 cm and length 65 cm in a closely spaced plate-finnedmatrix. Hot water enters the tubes at 90°C at a rate of 0.6 kg/s and leaves at65°C. Air flows across the radiator through the interfin spaces and is heatedfrom 20°C to 40°C. Determine the overall heat transfer coefficient Ui of thisradiator based on the inner surface area of the tubes.