A piece of copper of a mass 0.10kg, initially at 97.4°C, is dropped into 0.20 kg of water contained in a 0.28-kg aluminium can; the water and aluminium are initially at 15°C. What is the final temperature of the system? [Specific heat of water Cw-4190 J/kg°C; Specific heat of copper Car 385 J/kg°C: Specific heat of aluminium CA 900 J/kg°C] [Choose the closest answer] O a. None of the answer is correct O b. 32.19 Celsius O c. 15.00 Celsius O d. 11.17 Celsius O e. 17.81 Celsius What is the outside temperature if 4000 kcal of heat is lost through a 4.0 m² pane of 0.30 cm thick glass (k = 2.0x104 kcal/s m °C) in one hour from a house kept at 38°C? [hint: use the constant value provided]

A piece of copper of a mass 0.10kg, initially at 97.4°C, is dropped into 0.20 kg of water contained in a 0.28-kg aluminium can; the water and aluminium are initially at 15°C. What is the final temperature of the system? [Specific heat of water Cw-4190 J/kg°C; Specific heat of copper Car 385 J/kg°C: Specific heat of aluminium CA 900 J/kg°C] [Choose the closest answer] O a. None of the answer is correct O b. 32.19 Celsius O c. 15.00 Celsius O d. 11.17 Celsius O e. 17.81 Celsius What is the outside temperature if 4000 kcal of heat is lost through a 4.0 m² pane of 0.30 cm thick glass (k = 2.0x104 kcal/s m °C) in one hour from a house kept at 38°C? [hint: use the constant value provided]

Principles of Physics: A Calculus-Based Text

5th Edition

ISBN:9781133104261

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter17: Energy In Thermal Processes: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2OQ: A 100-g piece of copper, initially at 95.0C, is dropped into 200 g of water contained in a 280-g...

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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?
Equal masses of substance A at 10.0C and substance B at 90.0C are placed in a well-insulated container of negligible mass and allowed to come to equilibrium. If the equilibrium temperature is 75.0Q which substance has the larger specific heat? (a) substance A (b) substance B (c) The specific heats are identical. (d) The answer depends on the exact initial temperatures. (e) More information is required.
A certain ideal gas has a molar specific heat of Cv = 72R. A 2.00-mol sample of the gas always starts at pressure 1.00 105 Pa and temperature 300 K. For each of the following processes, determine (a) the final pressure, (b) the final volume, (c) the final temperature, (d) the change in internal energy of the gas, (e) the energy added to the gas by heat, and (f) the work done on the gas. (i) The gas is heated at constant pressure to 400 K. (ii) The gas is heated at constant volume to 400 K. (iii) The gas is compressed at constant temperature to 1.20 105 Pa. (iv) The gas is compressed adiabatically to 1.20 105 Pa.
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An ideal gas initially at 300 K undergoes an isobaric expansion at 2.50 kPa. If the volume increases from 1.00 m3 to 3.00 m3 and 12.5 kJ is transferred to the gas by heat, what are (a) the change in its internal energy and (b) its final temperature?
Consider the latent heat of fusion and the latent heat of vaporization for H2O, 3.33 105 J/kg and 2.256 106 J/kg, respectively. How much heat is needed to a. melt 2.00 kg of ice and b. vaporize 2.00 kg of water? Assume the temperatures of the ice and steam are at the melting point and vaporization point, respectively. (a). UsingEq21.9, Q = mLF = (2.00 kg) (3.33l05 J/kg) = 6.66105 J (b).UsingEq21.10. Q = mLV = (2.00kg) (2.256106 J/kg) = 14.51106 J
An aluminum rod 0.500 m in length and with a cross-sectional area of 2.50 cm2 is inserted into a thermally insulated vessel containing liquid helium at 4.20 K. The rod is initially at 300 K. (a) If one-half of the rod is inserted into the helium, how many liters of helium boil off by the time the inserted half cools to 4.20 K? Assume the upper half does not yet cool. (b) If the circular surface of the upper end of the rod is maintained at 300 K, what is the approximate boil-off rate of liquid helium in liters per second after the lower half has reached 4.20 K? (Aluminum has thermal conductivity of 3 100 W/m K at 4.20 K; ignore its temperature variation. The density of liquid helium is 125 kg/m3.)
Beryllium has roughly one-half the specific heat of water (H2O). Rank the quantities of energy input required to produce the following changes from the largest to the smallest. In your ranking, note any cases of equality, (a) raising the temperature of 1 kg of H2O from 20C to 26C (b) raising the temperature of 2 kg of H2O from 20C to 23C (c) raising the temperature of 2 kg of H2O from 1C to 4C (d) raising the temperature of 2 kg of beryllium from 1C to 2C (e) raising the temperature of 2 kg of H2O from -1C to 2C