Your calculator can't handle enormous exponents, but we canmake sense of large powers of e by converting them to largepowers of 10. If we write e = 10%, then eß = (10°)³ = 10³.Part AWhat is the value of a?απ17 ΑΣΦSubmitPart BRequest AnswerWhat is the multiplicity of a macrostate with entropy S = 1.0 J/K? Give your answer as a power of 10.Ω = 10αβ; αβ==)Π| ΑΣΦ

Answered: Image /qna-images/answer/1a832c4f-f946-40f8-aa6d-c94e7e916273.jpg

Your calculator can't handle enormous exponents, but we can make sense of large powers of e by converting them to large powers of 10. If we write e = 10°, then e = (10°)³ = 108. ▼ Part A What is the value of a? α = Submit Part B ΕΠΙ ΑΣΦ Request Answer What is the multiplicity of a macrostate with entropy S = 1.0 J/K? Give your answer as a power of 10. Ω = 10^β, αβ= ΠΫΠΙ ΑΣΦ ? 3 ?

Your calculator can't handle enormous exponents, but we can make sense of large powers of e by converting them to large powers of 10. If we write e = 10°, then e = (10°)³ = 108. ▼ Part A What is the value of a? α = Submit Part B ΕΠΙ ΑΣΦ Request Answer What is the multiplicity of a macrostate with entropy S = 1.0 J/K? Give your answer as a power of 10. Ω = 10^β, αβ= ΠΫΠΙ ΑΣΦ ? 3 ?

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

Chapter4: The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 87CP: A diatomic ideal gas is brought from an initial equilibrium state at p1=0.50 atm and T1=300K to a...

See similar textbooks

Similar questions

Experimental measurements of the heat capacity of aluminum at low temperatures (below about 50 K) can be fit to the formula Cv = aT+bT3 ,where Cv is the heat capacity of one mole of aluminum, and the constants a and b are approximately a = 0.00135 J/K2 and b = 2.48 X 10-5 J/K4. From this data, find a formula for the entropy of a mole of aluminum as a function of temperature. Evaluate your formula at T = 1 K and at T = 10 K, expressing your answers both in conventional units (J/K) and as unitless numbers (dividing by Boltzmann's constant).
Prove that the entropy of mixing of an ideal mixture has aninfinite slope, when plotted vs. x, at x = 0 and x = l.
A diatomic ideal gas is brought from an initial equilibrium state at p1=0.50 atm and T1=300K to a final stage with p2=0.20 atm and T1=500K. Use the results of the previous problem to determine the entropy change per mole of the gas.
In Debye Approximation the entropy at some temperature T (less than 10 K) is aT(Blank 1 ) /3 If the value of this entropy at T = 3.5 K is 1.55 J / K , then the value of the coefficient "a" is : ( Blank 2)
Hi, could I get some help with this macro-connection physics problem involving isothermal expansion? The set up is: For an isothermal reversible expansion of two moles of an ideal gas, what is the entropy change of the a) gas and b) the surroundings in J/K to 4 digits of precision if the gas volume quadruples, assuming NA = 6.022e23 and kB = 1.38e-23 J/K? Thank you.
Does the internal energy (U) of a perfect gas go up or down with increasing pressure under adiabatic, reversible conditions (i.e. at constant entropy)? Hint: you’re looking for ∂U/∂P)s . and under conditions of constant entropy, the transition must be adiabatic and reversible. As such: ∂U= CV ∂T, and ∂T/∂P )s = V/Cp
Show that during the quasistatic isothermal expansion of a monatomic ideal gas, the change in entropy is related to the heat input Q by the simple formula. SΔ= Q/TIn the following chapter I'll prove that this formula is valid for any quasistatic process. Show, however, that it is not valid for the free expansion process described above.
In this problem you are to consider an adiabaticexpansion of an ideal diatomic gas, which means that the gas expands with no addition or subtraction of heat. Assume that the gas is initially at pressure p0, volume V0, and temperature T0. In addition, assume that the temperature of the gas is such that you can neglect vibrational degrees of freedom. Thus, the ratio of heat capacities is γ=Cp/CV=7/5. Note that, unless explicitly stated, the variable γshould not appear in your answers--if needed use the fact that γ=7/5 for an ideal diatomic gas. Find an analytic expression for p(V), the pressure as a function of volume, during the adiabatic expansion. Express the pressure in terms of V and any or all of the given initial values p0, T0, and V0. p(V) = __________
In this problem you are to consider an adiabaticexpansion of an ideal diatomic gas, which means that the gas expands with no addition or subtraction of heat. Assume that the gas is initially at pressure p0, volume V0, and temperature T0. In addition, assume that the temperature of the gas is such that you can neglect vibrational degrees of freedom. Thus, the ratio of heat capacities is γ=Cp/CV=7/5. Note that, unless explicitly stated, the variable γshould not appear in your answers--if needed use the fact that γ=7/5 for an ideal diatomic gas. A) Find an analytic expression for p(V), the pressure as a function of volume, during the adiabatic expansion. Express the pressure in terms of V and any or all of the given initial values p0, T0, and V0. p(V) = __________ B) At the end of the adiabatic expansion, the gas fills a new volume V1, where V1>V0. Find W, the work done by the gas on the container during the expansion. Express the work in terms of p0, V0, and V1. Your…
In an experiment, 200 g of aluminum (with a specific heat of 900 J/kg K) at 100 C is mixed with 50.0 g of waterat 20.0C, with the mixture thermally isolated. (a) What is theequilibrium temperature? What are the entropy changes of (b) thealuminum, (c) the water, and (d) the aluminum–water system?
By how much does the entropy of 1.0 kg of water change when heated from 263.15 K up to 283.15 K at a pressure of 1 bar? (The solution is 1.5 kJ/K)
Show that the coefficients of performance of refrigerators and heat pumps are related by COPref = COPhp − 1 . Start with the definitions of the COP s and the conservation of energy relationship between Qh , Qc , and W .