Starting with the result of Problem 2.17, find a formula for the temperature of an Einstein solid in the limit qN. Solve for the energy as a function of temperature to obtain U=Nϵe-ϵ/kT (whereϵ is the size of an energy unit).

Short Answer

Expert verified

The required expression isU=Nεe-εkT.

Step by step solution

01

Given

Expression for the multiplicity of Einstein solid in low-temperature limit qNis given as:

role="math" localid="1646983518799" ΩNeqq..........(1)

Here, Nis number of oscillator in solid, qis number of energy unit.

02

Explanation

Mathematically, temperature can be defined as:

1T=SU..........(2)

Where,

Sis the change in entropy and Uis the change in the internal energy of the body.

Total energy of the system is given as:

U=qε

Where, qis number of energy unit.

Equation (1) can be written by substituting the values of qas:

ΩNeεUUε

Entropy is given as:

S=klnΩ

Here, kis Boltzmann constant and Ωis multiplicity.

By substituting the value of Ωin the above equation, we get,

S=klnNeεUUε

But lnab=bln(a), therefore, the above equation can be rewritten as:

S=kUεlnNeεU

Also, lnab=lna+lnband lnab=lna-lnbso, the above equation becomes:

S=UkεlnNε+lne-lnUS=UkεlnNε+1-lnU

By substituting this value of Sin equation (2), we get,

1T=SU=UUkεln(Nε)+1-ln(U)1T=kεln(Nε)+kε-UkUε-kεln(U)1T=kε[ln(Nε)-ln(U)]lnU=ln(Nε)-εkT

Take exponential for both the sides of the above equation,

U=elnNε-εkTU=eln(Nε)·e-εkTU=Nεe-εkT

This result is valid only for low temperature as U=qεN.

03

Final answer

Hence, the energy as a function of temperature can be solved to obtainU=Nϵe-ϵ/kT.

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Most popular questions from this chapter

The results of either of the two preceding problems can also be applied to the vibrational motions of gas molecules. Looking only at the vibrational contribution to the heat capacity graph for H2shown in Figure 1.13, estimate the value of εfor the vibrational motion of anH2 molecule.

What partial-derivative relation can you derive from the thermodynamic identity by considering a process that takes place at constant entropy? Does the resulting equation agree with what you already knew? Explain.

A cylinder contains one liter of air at room temperature ( 300K) and atmospheric pressure 105N/m2. At one end of the cylinder is a massless piston, whose surface area is 0.01m2. Suppose that you push the piston in very suddenly, exerting a force of 2000N. The piston moves only one millimeter, before it is stopped by an immovable barrier of some sort.

(a) How much work have you done on this system?

(b) How much heat has been added to the gas?

(c) Assuming that all the energy added goes into the gas (not the piston or cylinder walls), by how much does the internal energy of the gas increase?

(d) Use the thermodynamic identity to calculate the change in the entropy of the gas (once it has again reached equilibrium).

Consider an Einstein solid for which both N and q are much greater than 1. Think of each oscillator as a separate "particle."

(a) Show that the chemical potential is

role="math" localid="1646995468663" μ=-kTlnN+qN

(b) Discuss this result in the limits Nqand Nq, concentrating on the question of how much Sincreases when another particle carrying no energy is added to the system. Does the formula make intuitive sense?

Use a computer to reproduce Table 3.2 and the associated graphs of entropy, temperature, heat capacity, and magnetization. (The graphs in this section are actually drawn from the analytic formulas derived below, so your numerical graphs won't be quite as smooth.)

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