A vessel has two identical compartments (e.g. left and right), but gas moleculescan go from each compartment into the other.(a) Initially there are 12 molecules in the left compartment and 0 molecules in the rightcompartment. Finally there are 6 molecules in the left compartment and 6 moleculesin the right compartment. What happens with the total entropy of the gas in such aprocess?(b) Is it possible that the gas can go spontaneously from 6 molecules in the left compart-ment, 6 molecules in the right compartment to 12 molecules in the left compartment,0 molecules in the right compartment?

Entropy: A more random and less ordered movement of molecules without set locations or orientations…

Answered: A vessel has two identical compartments…

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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Two moles of an ideal gas undergo an irreversible isothermal expansion fromVa=100 liters to Vb=300 liters at T=300K.(a) What is the entropy change for this process?(b) What is the Gibbs free energy change?(c) Is this process spontaneous or not? Explain your answer.
A 0.50-kg piece of aluminum at 250 °C is dropped into 1.0 kg of water at 20 °C . After equilibrium is reached, what is the net entropy change of the system?
Suppose you put a cube of ice of mass 100 g into a glass of water at just above 0°C. When the ice melts, about 33 kJ of energy is absorbed from the surroundings as heat. What is the change in entropy of (a) the sample (the ice) and (b) the surroundings (the glass of water)?
When a metal bar is temporarily connected between a hot reservoir at Th and a cold reservoir at Tc, the energy transferred by heat from the hot reservoir to the cold reservoir is Qh. In this irreversible process, find expressions for the change in entropy of the following. (Use any variable or symbol stated above as necessary.) (a) the hot reservoir ΔSh = (b) the cold reservoir ΔSc = (c) the Universe ΔSU =
What would happen to the entropy of a system if you could increase the pressure without changing the temperature, volume, or number of particles?
(a) What is the unit of "specific entropy"? Is it an extensive property? (b) What is an isentropic process? Please give an example. (c) Explain the increase of entropy principle. (d) The entropy of a hot baked pizza decreases as it cools. Is this a violation of the increase of entropy principle? Explain.
Consider the adiabatic free expansion of n moles of an ideal gas from volume V₁ to volume V2, where V₂ > V₁. [Hint: check lecture 19, chapter 5.6, process number 5. Note that such a process happens quasi-instantaneously, thus, it is irreversible.] (1) Calculate the change in entropy of the gas. (2) Calculate the change in entropy of the environment. (3) Evaluate the total change in entropy (AS = ASgas + ASenv.) for 1 mole, with V₂ = 2V/₁.
A box contains 100 gas molecules all released on the left side of the box. What is the initial entropy of all the gas molecules on one side? You can calculate the number of microstates (left/right distribution of molecules) possible by the equation W = N! / ( nL! * nR!,) where N is the total number of molecules and nL is the number on the left and nR is the number on the right. What is the entropy of the most disorganized distribution of gas molecules?
A rigid box contains 0.9 mol of an ideal monoatomic gas. Heat is added to the gas and its temperature changes from 183 K to 295 K. If this is a reversible process, what is the change in entropy of the gas in J/K?
Suppose that 10 distinguishable particles are equipartitioned in a container that has 100 equal-sized compartments. What is the entropy on this system?

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