Suppose there are 10 distinguishable particles in a box divided into two equal compartments, A and B. What is the change in entropy of the system when compartments (A, B)'s particles were changed from (na = 8,ng = 2) to (nA = 6.ng = 4) respectively in terms of k, the Boltzmann constant? %3! %3D A. -4.67k В. - 1.54к С. 1.54к D. 4.67k

Suppose there are 10 distinguishable particles in a box divided into two equal compartments, A and B. What is the change in entropy of the system when compartments (A, B)'s particles were changed from (na = 8,ng = 2) to (nA = 6.ng = 4) respectively in terms of k, the Boltzmann constant? %3! %3D A. -4.67k В. - 1.54к С. 1.54к D. 4.67k

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

Chapter4: The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 63P: A monoatomic ideal gas (n moles) goes through a cyclic process shown below. Find the change in...

See similar textbooks

Similar questions

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.
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
A copper rod of cross-sectional area 5.0 cm2 and length 5.0 m conducts heat from a heat reservoir at 373 K to one at 273 K. What is the time rate of change of the universe's entropy for this process?
(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?
(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 system consisting of n moles of an ideal gas with molar specific heat at constant pressure Cr undergoes two reversible processes. It starts with pressure Pi and volume Vi, expands isothermally, and then contracts adiabatically to reach a final state with pressure Pi and volume 3Vi. (a) Find its change in entropy in the isothermal process. (The entropy does not change in the adiabatic process.) (b) What If? Explain why the answer to part (a) must be the same as the answer to Problem 46. (You do not need to solve Problem 46 to answer this question.)
A sample of a monatomic ideal gas is contained in a cylinder with a piston. Its stale is represented by the dot in the PV diagram shown in Figure OQ22.9. Arrows A through E represent isobaric, isothermal, adiabatic, and isovolumetric processes that the sample can undergo. In each process except D, the volume changes by a factor of 2. All five processes are reversible. Rank the processes according to the change in entropy of the gas from the largest positive value to the largest-magnitude negative value. In your rankings, display any cases of equality.
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.
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.