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We have repeatedly stressed
the fact that whenever you encounter Boltzmann's constant k we deal with the particle unit "atom" or
"molecule", while whenever we encounter the gas constant R, we deal with the the unit "mol".
Here we will quickly survey the connection. |
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First we have the general law for ideal gases with volume V, pressure p
and temperature T |
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This was first an empirical law that later became fully understood by statistical thermodynamics. |
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The next step is to realize that if you increase the volume while keeping everything
else constant, the "const" in the law must increase in the same proportion. This leads to the much more universal
formulation that is generally used: |
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With n = quantity of the gas, and R = gas constant with a value depending
on how you measure n. |
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This would still leave room for R being different for different kind of
gases. Avogadro enters, proposing that identical volumina of
gases under identical pressure and temperature contain identical numbers of particles. |
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This permits to define R for all (ideal) gases and to measure it. We find |
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| R | = |
p · V
nmol · T |
= |
8.32441 J · K–1 · mol–1 |
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if me measure the quantity n of the gas in mols.
º |
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One mol
of a substance, per definition, contains just as many particles, objects, or
building blocks of that substance (i.e. atoms, molecules, electrons, vacancies, ...), as there are carbon atoms in 1
g of 12C which gives |
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Avogadros constant then automatically is |
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i.e. we have 6.022 · 1023 particles per mol
of a substance. |
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If we set n = 1 we have for the mol-volume Vm,
i.e. for the volume that 1 mol of a gas occupies |
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| Vm | = |
n · R · T
p |
= 22.414 | l
mol |
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This is valid for for "old" standard conditions (p = 1013
mbar = 101 325 Pa, and T = 0oC ). |
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For the "new" standard conditions (p = 100 000 Pa, T = 298.15 K)
we have Vm = 24.789 l/mol |
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Why the international standards and units of measurements must change all the time is beyond me, but
that's the way it is. I have suffered through 4 changes in the units for pressure by now, not to mention the big
pain caused by the fact that the Americans normally don't care and still stick to psi. |
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If we now measure substance quantities not per mol, but per particle, we must
divide R by Avogadros constant NA and obtain |
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| p·V | = |
npart · |
R
NA |
· T = npart · kT |
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and npart is now the number of particles
in V. |
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For R/NA
=: k = Boltzmann's constant we obtain |
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| k | = |
8.32441
6.022 · 1023 |
| J · K–1 |
= 8.616 · 10–5eV · K–1 |
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Fine, we can see that as a definition of Boltzmann's
constant k. But now we have two questions: |
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1. Why is the k from the gas law the same number as in the famous entropy equation S = k · ln P ? |
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Not obvious - and not exactly easy to prove. Essentially, you have to unleash the full
power of statistical thermodynamics to show that both k's are identical. So either grab your thermodynamic textbook,
or believe your professor at this point. |
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2. Is there a way to calculate the numerical value of k from some more fundamental
constants? Well, as far as I know, it cannot be done. So k is a basic constant of nature, in the same league as other fundamental constants of nature, like the speed
of light, the gravitational constant, or the elementary charge. |
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Finally something to make things really complicated: |
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Changing from mols to particle
numbers or densities, changes the precise formulation of the mass action
law. Consult the link for details. |
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© H. Föll (Defects - Script)
Internal Energy, Enthalpie, Entropy and Free Enthalpie 
With frame