55 g of aluminum at 100° C are placed in thermal contact with 55 g of copper at 0° C. The two metals are isolated from the environment. As the metals reach thermal equilibrium, what is the entropy change of the aluminum? Express your answer with the appropriate units. ASAL= Submit Part B AScu= Submit Part C μA Value As the metals reach thermal equilibrium, what is the entropy change of the copper? Express your answer with the appropriate units. Request Answer ASuniverse = μÀ Value Request Answer O " μÃ Units As the metals reach thermal equilibrium, what the entropy change of the universe? Express your answer to two significant figures and include the appropriate units. Value 1 Units ? Units ? ?

55 g of aluminum at 100° C are placed in thermal contact with 55 g of copper at 0° C. The two metals are isolated from the environment. As the metals reach thermal equilibrium, what is the entropy change of the aluminum? Express your answer with the appropriate units. ASAL= Submit Part B AScu= Submit Part C μA Value As the metals reach thermal equilibrium, what is the entropy change of the copper? Express your answer with the appropriate units. Request Answer ASuniverse = μÀ Value Request Answer O " μÃ Units As the metals reach thermal equilibrium, what the entropy change of the universe? Express your answer to two significant figures and include the appropriate units. Value 1 Units ? Units ? ?

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

Chapter18: Heat Engines, Entropy, And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 10OQ: Assume a sample of an ideal gas is at room temperature. What action will necessarily make the...

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An ideal gas is taken from an initial temperature Ti to a higher final temperature Tf along two different reversible paths. Path A is at constant pressure, and path B is at constant volume. What is the relation between the entropy changes of the gas for these paths? (a) SA SB (b) SA = SB (c) SA SB
Assume a sample of an ideal gas is at room temperature. What action will necessarily make the entropy of the sample increase? (a) Transfer energy into it by heat. (b) Transfer energy into it irreversibly by heat. (c) Do work on it. (d) Increase either its temperature or its volume, without letting the other variable decrease. (e) None of those choices is correct.
(a) What is the change in entropy if you start with 100 coins in the 45 heads and 55 tails macrostate, toss them, and get 51 heads and 49 tails? (b) What if you get 75 heads and 25 tails? (c) How much more likely is 51 heads and 49 tails than 75 heads and 25 tails? (d) Dues either outcome violate the second law of thermodynamics?
Two hundred grams of water at 0 is brought into contact into thermal equilibrium successively with reservoirs at 20 , 40 , 60 , and 80 . (a) What is the entropy change of the water? (b) Of the reservoir? (c) What is the entropy change of the universe?
An ideal gas is taken from an initial temperature Ti to a higher final temperature Tf along two different reversible paths as shown in Figure 21.15. Path A is at constant pressure, and path B is at constant volume. What is the relation between the entropy changes of the gas for these paths? (a) SA SB (b) SA = SB (c) SA SB Figure 21.15 (Quick Quiz 21.5) An ideal gas is taken from temperature Ti to Tf via two different paths.
An athlete whose mass is 70.0 kg drinks 16.0 ounces (454 g) of refrigerated water. The water is at a temperature of 35.0F. (a) Ignoring the temperature change of the body that results from the water intake (so that the body is regarded as a reservoir always at 98.6F), find the entropy increase of the entire system. (b) What If? Assume the entire body is cooled by the drink and the average specific heat of a person is equal to the specific heat of liquid water. Ignoring any other energy transfers by heat and any metabolic energy release, find the athletes temperature after she drinks the cold water given an initial body temperature of 98.6F. (c) Under these assumptions, what is the entropy increase of the entire system? (d) State how this result compares with the one you obtained in part (a).
(a) What is the change in entropy if you start with 10 coins in the 5 heads and 5 tails macrostate, toss them, and get 2 heads and 8 tails? (b) How much more likely is 5 heads and 5 tails than 2 heads and 8 tails? (Take the ratio of the number of microstates to find out.) (c) If you were betting on 2 heads and 8 tails would you accept odds of 252 to 45? Explain Why or why not. Table 15.5 10Coin Toss MacrostateNumber of Microstates (W) Heads Tails 10 0 1 9 1 10 8 2 45 7 3 120 6 4 210 5 5 252 4 6 210 3 7 120 2 8 45 1 9 10 0 10 1 Total: 1024
A monoatomic ideal gas (n moles) goes through a cyclic process shown below. Find the change in entropy of the gas in each step and the total entropy change over the entire cycle.
A sealed container holding 0.500 kg of liquid nitrogen at its boiling point of 77.3 K is placed in a large room at 21.0C. Energy is transferred from the room to the nitrogen as the liquid nitrogen boils into a gas and then warms to the rooms temperature. (a) Assuming the rooms temperature remains essentially unchanged at 21.0C, calculate the energy transferred from the room to the nitrogen. (b) Estimate the change in entropy of the room. Liquid nitrogen has a latent heat of vaporization of 2.01 105 J/kg. The specific heat of N2 gas at constant pressure is CN2 = 1.04 103J/kg K.
The Carnot cycle is represented by the temperature-entropy diagram shown below. (a) How much heat is absorbed per cycle at the high-temperature reservoir? (b) How much heat is exhausted per cycle at the low-temperature reservoir? (c) How much work is done per cycle by the engine? (d) What is the efficiency of the engine?
A cylinder contains 500 g of helium at 120 atm and 20 . The valve is leaky, and all the gas slowly escapes isothermally into the atmosphere. Use the results of the preceding problem to determine the resulting change in entropy of the universe.