References
This summary is based mainly on two papers:
Hydrogen Atom Bond Increments for Calculation of Thermodynamic Properties of Hydrocarbon Radical Species, Tsan H. Lay, Joseph W. Bozzelli, Anthony M. Dean, and Edward R. Ritter, J. Phys. Chem. 1995, 99, 39, 14514–14527: This paper outlines the original implementation of THERM.
Energy Levels and Thermodynamic Functions for Molecules with InternalRotation I. Rigid Frame with Attached Tops, Kenneth S. Pitzer and William D. Gwinn, J. Chem. Phys. 10, 428 (1942): This paper used for the table for conversion of Moments of Inertia (Ir) and Torsion Barriers (V) to entropy.
Information and Summary found in THERM paper
This summary follows the example in the THERM paper.
In THERM and THERGAS, to calculate the thermodynamics of a radical, they calculate the parent molecule and then examine the loss/gain (among other things) due to the formation of the radical. If you look at Table 5 of Bozzelli's THERM, you can see the corrections due to the formation of the radical (he collects all these corrections in one HBI term --- these are in Table 5).
For calculation of CCJ, see Table 5, the first set, there is a loss of the CH3-CH3 rotor and a gain of the CH3-CH2. rotor. The Ir and V value should be used to calculate the correction to the Entropy (and heat capacities):
rotor - CH3-CH3:: -3.864 cal/(mol K)
rotor - CH3-CH2: 4.756 cal/(mol K)
From the THERM paer (pg 14518 - Section 'Hindered Internal Rotations'):
The differences in the entropy of internal rotation between parent (molecule) and daughter (radical) resulting from changes in rotational barriers and moments of inertia are usually the major components of the entropy increment in HBI groups. The method and tables of Pitzer and Ginn are used to calculate the contribution of hindered internal rotations to the thermodynamic functions SO298 and Cp(T);
From the THERM paper (pg 14518 - Section 'Hindered Internal Rotations'):
The barriers of hindered internal rotations for stable molecules and free radicals considered in this work are listed in Table 4.
From Table 4: Moments of Inertia (Ir) and Torsion Barriers (V) for the hindered rotations about single bonds:
CH3-CH3 Ir=1.6 V=2.9
RCH2-CH3 Ir=3.0 V=3.3
CH3-CH2 Ir= 1.2 V=0.1
RCH2-CH2 Ir=0.1 V=2
From the Appendix of the THERM paper (pg 14526):
There is no simple equation to express S(int-rot) and Cp(int-rot). These parameters are calculated using the method and tables of Pitzer and Gwinn . Two parameters are needed to utilize the tables of Pitzer and Gwinn in this calculation of S(int-rot) and CP(int-rot): V (actually V/RT) and l/Qf. V is the potential barrier, R is the ideal gas constant, T is temperature, and Qf is the partition function of free rotation and is given by
Q, = (8 (pi)**3 Ir k T)**(1/2)/(hn)
where Z, is the reduced moment of inertia, k is Boltzmann's constant, and n is the number of potential minima per revolution. The calculation of Qf and the interpolation of Pitzer and Gwinn's tables to obtain the entropy and heat capacity values are implemented (automated) by a computer code. Table IV (in ref 32 for entropy decrease from classical free rotation is incorporated into the code and used to calculate the entropy values. Table VI therein is used to calculate the heat capacities.
In Benson's book, in the notes of Table A.16, the formula for Q is given as:
Q = 3.6/(sigma)* (Ir T/100)**2
For CH3-CH3 and CH3-CH2 this is 2.62 and 2.26, respectively. This give 1/Qf values of 0.38 and 0.29, respectively.
'Reproduction' of example given in the Appendix of THERM paper
From the Appendix of THERM paper (pg 145526):
Using CH3-CH3 as an example, Ir of this symmetric coaxial CH3 rotor can be calculated from
lr = 1/I1 + 1/I2
where I1 and I2 are the moments of inertia of each methyl top. Ir is 1.6 amu A*, and Qf is then calculated as 2.62. With the rotational barrier equal to 2.9 kcal/mol, the entropy contribution is calculated, from use of the tables, as 3.86 cal/(mol K) at 298K. The reduced moment of inertia for rotation of the CH2 group in the ethyl radical is calculated as 1.2 amu A2, and with the barrier of 0.1 kcal/mol, the internal rotational entropy contribution at 298 K is obtained as 4.76 cal/(mol K).
My Calculations for CH3-CH3
In my own calculations for CH3-CH3, Ir=1.6, which means Q=2.62 (same as in the above in the THERM paper). 1/Q is 0.38.
V is 2.9 (from Table 4 of THERM paper). V/RT=2900/(1.9869*298)=4.90
Using Table III (TABLE III. Entropy, S (cal. per degree mole). ) in Gwinn and Pitzer to translate to S value. Extrapolating between the table values, we get (S-Sf)=0.657:
Q=0.40 V/RT=5.0 (S-Sf)=1.235
Q=0.35 V/RT=5.0 (S-Sf)=1.281
Q=0.40 V/RT=4.5 (S-Sf)=1.116
Q=0.35 V/RT=4.5 (S-Sf)=1.153
1.235 - (1.281-1.235)*( (0.40-0.38)/(0.40-0.35))=1.263
1.116 - (1.153-1.116)*( (0.40-0.38)/(0.40-0.351.234))=1.138
1.263 - (1.263-1.138)*( (5.0-4.9)/(5.0-4.5) )=
1.236*3=3.70
However, this does come close to the value of 3.86 (from THERM paper: the entropy contribution is calculated, from use of the tables, as 3.86 cal/(mol K) at 298K.), but it is not exact. In addition, the number 3.86/3=1.29 is outside the range of numbers possible for the values of 1/Qf=0.38 and V/RT=4.90.
Same Calculation for CH3-CH2
For CH3-CH2 Ir=1.2 which means:
Q=Q = 3.6/(sigma)* (Ir T/100)**(1/2) = 3.6/6*(1.2 *298/100)**(1/2) = 1.135,
Q=Q = 3.6/(sigma)* (Ir T/100)**(1/2) = 3.6/2*(1.2 *298/100)**(1/2) = 3.404,
giving 1/Qf=0.88 (or 0.293 for sigma=2).
V is 0.1 (from Table 4 of THERM paper).
V/RT=100/(1.987*298)=0.169
The value from the table for 1/Q=0.88 V=0.169 looks like it is close to zero (even when multiplied by 6).
(The value from the table for 1/Q=0.293 V=0.169
This is not close to the value given in Table 5 of the THERM paper of 4.756. The value close to zero is closer to the THERGAS assumption that the only contribution is loss of the rotation from the parent.
For RCH2-CH3 Ir=3.0 which means:
Q=Q = 3.6/(sigma)* (Ir T/100)**(1/2) = 3.6/3*(3.0 *298/100)**(1/2) = 3.588 ,
giving 1/Qf= 0.279
V is 3.3 (from Table 4 of THERM paper).
V/RT=3300/(1.987*298)=5.573
The point is: 1/Q=0.279 V=5.573
From the table
1/Q=0.4 V=6.0 E=1.444 1.444*3 = 4.332
1/Q=0.35 V=5.0 E=1.218 1.218*3 = 3.654
This is sort of close to the value given in Table 5 of the THERM paper of 4.283.
Value of constants cm-g-s-K units from http://www.physics.rutgers.edu/~abrooks/342/constants.html
Conversion of Ir to Qf at a given temperature
Staring point equation on page 14526 in the Appendix of the THERM paper
The derived formula does not match the formula given in Benson's book from info in Table A.16:
3.6/n ( (Ir T)/100)**2
my derived formula is basically a factor of 10 too big (factor of 100 in square root).
From the Table 5 of THERM paper
CH3CH3 Erot = 3.864 sigma=3
CH3CH2 Erot= 4.756 sigma=6
RCH2CH3 Erot = 4.283 sigma = 3
RCH2CH2 Erot = 5.183 sigma =2
This means from the (V/RT,Qf) tables there should be a value of:
CH3CH3 3.864/3=1.288
CH3CH2 4.756/6=0.7927
CH3CH3 Ir=1.6 V=2.9 n=3 Sf= 3.468
CH3CH2 Ir=1.2 V=0.1 n=6 Sf= 3.386
RCH2CH3 Ir=3.0 V=3.3 n=3 Sf= 3.502
RCH2CH2 Ir=1.8 V=0.1 n=2 Sf= 3.800