Imagine a particle that can be in only three states, with energies -0.05 eV, 0, and 0.05 eV. This particle is in equilibrium with a reservoir at 300 K.

(a) Calculate the partition function for this particle.

(b) Calculate the probability for this particle to be in each of the three states.

(c) Because the zero point for measuring energies is arbitrary, we could just as well say that the energies of the three states are 0, +0.05 eV, and +0.10 eV, respectively. Repeat parts (a) and (b) using these numbers. Explain what changes and what doesn't.

Short Answer

Expert verified

Therefore,

(a) the partition function is Z=8.063

(b) the probability for this particle is P1=0.858P2=0.124P3=0.018

(c)Z=1.165P1=0.858P2=0.124P3=0.018

Step by step solution

01

Given information

A particle that can be in only three states, with energies -0.05 eV, 0, and 0.05 eV. This particle is in equilibrium with a reservoir at 300 K.

02

Explanation

(a) The partition function is equal to the total of all Boltzmann factors, i.e.

Z=se-E(s)/kT

Consider a particle that can exist in three states, each with an energy of ϵ1=-0.05 eV, ϵ2= 0 eV, and ϵ3= 0.05 eV; the partition function is:

Z=e-ϵ1/kT+e-ϵ2/kT+e-ϵ3/kT

Substitute the energies and Boltzmann's constant

Z=e0.05eV/0.025851eV+e0+e-0.05eV/0.025851eVZ=8.063

(b)The probability is given by:

P=1Ze-E(s)/kT

For first state,

P1=1Ze-ϵ1/kT=18.063e0.05eV/0.025851eVP1=0.858

For second state,

P2=1Ze-ϵ2/kT=18.063P2=0.124

For third state,

P3=1Ze-ϵ3/kT=18.063e-0.05eV/0.025851eVP3=0.018

03

Explanation

(c) Now imagine a particle that can exist in three states with energies of ϵ1= 0 eV, ϵ2= 0.05 eV, and ϵ3= 0.10 eV; the partition function is:Z=e-ϵ1/kT+e-ϵ2/kT+e-ϵ3/kT

Substitute with energies and Boltzmann's constant:

role="math" localid="1647298423935" Z=e0+e-0.05eV/0.025851eV+e-0.10eV/0.025851eVZ=1.165

For first state

P1=1Ze-ϵ1/kT=11.165P1=0.858

For second state:

P2=1Ze-ϵ2/kT=11.165e-0.05eV/0.025851eVP2=0.124

For third state

P3=1Ze-ϵ3/kT=11.165e-0.10eV/0.025851eVP3=0.018

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Most popular questions from this chapter

Consider a hypothetical atom that has just two states: a ground state with energy zero and an excited state with energy 2 eV. Draw a graph of the partition function for this system as a function of temperature, and evaluate the partition function numerically at T = 300 K, 3000 K, 30,000 K, and 300,000 K.

In the low-temperature limit (kT<<), each term in the rotational partition function is much smaller than the one before. Since the first term is independent of T, cut off the sum after the second term and compute the average energy and the heat capacity in this approximation. Keep only the largest T-dependent term at each stage of the calculation. Is your result consistent with the third law of thermodynamics? Sketch the behavior of the heat capacity at all temperature, interpolating between the high-temperature and low- temperature expressions.

Prove that the probability of finding an atom in any particular energy level is P(E)=(1/Z)e-F/kT, whereF=E-TS and the "'entropy" of a level is k times the logarithm of the number of degenerate states for that level.

In the numerical example in the text, I calculated only the ratio of the probabilities of a hydrogen atom being in two different states. At such a low temperature the absolute probability of being in a first excited state is essentially the same as the relative probability compared to the ground state. Proving this rigorously, however, is a bit problematic, because a hydrogen atom has infinitely many states.

(a) Estimate the partition function for a hydrogen atom at 5800 K, by adding the Boltzmann factors for all the states shown explicitly in Figure 6.2. (For simplicity you may wish to take the ground state energy to be zero, and shift the other energies according!y.)

(b) Show that if all bound states are included in the sum, then the partition function of a hydrogen atom is infinite, at any nonzero temperature. (See Appendix A for the full energy level structure of a hydrogen atom.)

(c) When a hydrogen atom is in energy level n, the approximate radius of the electron wavefunction is a0n2, where ao is the Bohr radius, about 5 x 10-11 m. Going back to equation 6.3, argue that the PdV term is Tot negligible for the very high-n states, and therefore that the result of part (a), not that of part (b), gives the physically relevant partition function for this problem. Discuss.

The analysis of this section applies also to liner polyatomic molecules, for which no rotation about the axis of symmetry is possible. An example is CO2, with =0.000049eV. Estimate the rotational partition function for a CO2molecule at room temperature. (Note that the arrangement of the atoms isOCO, and the two oxygen atoms are identical.)

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