# New Semiempirical Equation Describing Evaporation and Condensation in Nonassociated Liquids

Authors: Mihail Yu. Gorbachev; Anatholy S. Dimoglo
Journal: Journal of Chemistry
 (2013)

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## Abstract

The consideration of the evaporating and condensing molecules’ interaction with the surface layer of nonassociated liquids made it possible to find an equation for relations between the saturated vapor pressureP, from one side, and surface tension, critical temperature, and molar volume of the liquids, from the other side. This equation takes into account the influence of intramolecular conformational transitions of evaporating molecules on the quantity of their energy barrier. There are two types of the condensation process for the nonassociated liquids: soft and hard molecular condensation. For some vapor molecules the surface layer of the liquids behaves as an impenetrable elastic film. In the case of evaporating molecules, their one-particle potential barrier caused by the surface molecules vibration is essentially higher for the conformationally flexible molecules than that for rigid ones.


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## Body

## 1. Introduction

For nonassociated liquids in the state of phase equilibrium with their saturated vapor, both evaporation and condensation are responsible for the level of the vapor pressure. In its turn, the saturated vapor pressure of liquids (P) is related also to the intensity of molecular motion (i.e., molecular kinetic temperature) therein. And really, any increase in absolute temperature T of a liquid leads to the corresponding increase in the motion intensity, when the number of molecules evaporating per unit time from the unit surface (and, therefore, value of P) grows [1].Usually the dependence ofP on T can be described by means of the following equation (Antoine’s equation [2]):
(1)lnP=A-B(T+C).In (1) A, B, and C are some constants which differ for various liquids. As a rule, for any liquid these constants are being defined on the basis of its experimental P values. Other numerous correlations between lnP and T are similar to (1), and they are formed by means of various additional addenda depending on T to its right-hand side (see [3]). However, any above-mentioned correlation applied to the calculation of P for a new liquid requires the definition of its own new constants depending on the nature of this new liquid.Furthermore, it is well known that molecules of any liquid can be divided into two groups, according to the value of their one-particle kinetic energy [1]. The first group includes the so-called “hot” molecules. Their kinetic energy is greater than or equals to some critical for jumping value E. The molecules of the second group stay in their potential wells caused by the intermolecular attractive forces between these molecules. The given molecules take part in their vibration motion. The relative share z of the molecules of the first group may be found by means of the Boltzmann statistics [1]:
(2)z=exp(-EkT),
where k is the Boltzmann constant and E is the above-mentioned critical value of one-particle energy.If we consider the investigated molecules as spherical particles, whose effective radius is proportional toV1/3 (V is the molar volume of a liquid), then the following equation holds for the quantity E [4, 5]:
(3)E=fσV2/3,
where σ denotes the surface tension of a liquid, and f is a coefficient of proportionality, which is constant for many liquids (i.e., does not depend on T) [4, 5]. Then the relative share z of the above-mentioned jumping molecules (the first group) can be defined by means of the following equation:
(4)z=exp(-gσV2/3T).In (4) g is a constant (g=f/k) equal to 9.35×106 (J−1 K mol2/3) for various nonassociated liquids.Some part of these jumping molecules can escape the investigated liquid phase and immediately form vapor phase [1]. It has also been shown [4] that the thermal kinetic energy of a nonassociated liquid (and, therefore, its value of P) increases with the increase of z value. Bearing in mind all the above reasons, the aim of the present work is to find an equation that relates the quantity P with the share z of jumping molecules.


## 2. Methods of Calculations

### 2.1. Method of Calculations Evaporation in Nonassociated Liquid

In order to find the above equation, let us consider one mole of a liquid with conformationally rigid molecules. Hereinafter we suppose that the given liquid is in thermal equilibrium with its saturated vapor (its temperatureT is within the interval between its normal freezing and normal boiling points). We shall consider all the molecules of the investigated liquid as spherical particles (hard spheres) due to their fast mutual reorientations. The above value of T is supposed to be high enough for the consideration to be valid.Here it is to be noted that the share of the evaporating molecules of this liquid is less than that of the molecules jumping within its volume. It has been shown [6] that the surface layer of any nonassociated liquid is formed of its vibrating molecules.Here, vibrating molecules are molecules of liquids with weight centres staying for a while in their potential wells formed by neighbouring molecules. Vibrating molecules may become jumping ones andvice versa, but they have also a period of “settled life,” which allows for considering them as vibrating molecules.Thus, molecules abandoning the liquid phase must have high enough values of their one-particle kinetic energy in order to get over the potential barrierL caused by the vibrating molecules belonging to the surface layer. As far as the energy well of a vibrating molecule is proportional to σV2/3 (see (3)), hereinafter we shall consider that the quantity L may be described by means of the following equation:
(5)L=lσV2/3.Equation (5) is similar to (3); however, there is a principal difference between them. The coefficient l in (5) may depend on T and on the nature of the investigated liquid phase as well. In other words, the quantity L is proportional to the energy of the one-particle potential well and also may depend on the structure of the surface layer, namely, its thickness which is being defined by the chemical nature of its vibrating molecules and the value of T of the given liquid phase. If one-particle kinetic energy of a jumping molecule is higher than the above mentioned its critical value L, the molecule will be capable of escaping liquid phase. The relative share s of such molecules may be found by means of the Boltzmann statistics [1]:
(6)s=exp(-LkT)=exp(-æσV2/3T),
where æ(æ=l/k), in its turn, depends on T and the nature of the liquid phase.For different non-associated liquids it was shown [6] that molecules in their near-surface layers form a peculiar quasi crystal phase. This phase is being formed for the account of jumping molecules quitting the near-surface layers when passing to the gas phase. By this, the temperature of these layers becomes lower than that in the whole volume of the liquid.The molecules of near-surface layers participate mainly in vibrational but not in jumping motion. Only they are responsible, from one part, for the surface tension phenomena in such liquids, and from the other part, namely, they form a potential barrier for evaporating or condensing molecules. The order in the given quasi crystal phase grows while nearing the surface layer of the liquid. From the liquid part, this area is messy enough, and its border is diffusive. In this work we suppose that the volume concentration of molecules in this area is practically equal to their concentration in the whole volume.Now, let the total number of all jumping molecules be equal tozNa (Na is Avogadro’s number) and let their volume concentration in the given liquid phase be n=zNa/V. Then the number C of collisions (per unit time) among the above-mentioned jumping molecules with energies greater than or equal to L and the vibrating ones situated on some unit area of the surface layer may be defined from the equation below [1]:
(7)C=n(kT2πm)1/2exp(-LkT)=(zNaV)(kT2πm)1/2exp(-æσV2/3T),
where m is the molecular mass of one molecule and the quantity z is being defined by means of (4). At the same time, C will be also equal to the number of evaporating jumping molecules, which are capable of quitting the investigated liquid through its unit surface per unit time (because their energy is high enough for getting over the surface layer).


### 2.2. Describing Condensation in Nonassociated Liquids

Now let us consider the inverse process of molecular condensation as passing from the saturated vapor phase into the considered liquid one. Hereinafter we shall suppose that the process can be divided into two simultaneous processes. The first one is the condensation of those vapor molecules, whose one-particle kinetic energy is less than or equal to the above-mentioned critical energyE (see (3)). In this case, attractive forces between vapour molecules and vibrating surface molecules are capable of fixing the former ones on the surface of the liquid. The number D of the vapor molecules that are being fixed on the area unit of this surface per unit time may be easily found by means of the following equation [1]:
(8)D=γ(kT2πm)1/2[1-exp(-EkT)]=γ(kT2πm)1/2(1-z),
where γ is the value of the total volume’s concentration for the molecules of the liquid under study in its saturated vapor phase. As far as for the considered fixed vapor molecules the critical value of one-particle kinetic energy E is being defined by (3); our (8) contains z as its parameter (see (4)). However, it should be noted that in (8) z denotes the relative share of those vapor molecules which can be fixed on the liquid surface due to the intermolecular attractive forces. The condensation of such “slow” molecules may be called as “soft” condensation.The presence of quasi-crystal area consisting of a few surface layers of the liquid (see [6]) is the reason of the fact that molecules moving to the surface layer (from either gas phase or liquid phase) must necessarily be influenced by a potential that has been formed by the molecules of the quasi-crystal area. This potential (from both sides of the very surface layer) will look like a Morse curve. However, the Morse curve, be it nearby the layer or in departure of it, can be represented by two parabolas, one for the area of minimum and the other for the more distant area. Thus, the energy of the quitting the surface level molecules will be described by two squared members being kinetic and potential energies of their interaction with quasi crystal molecules. According to the introduced approximation, potential energy of a molecule will quadratically depend on its distance till the very surface layer.In this way, square roots will appear nowhere (including the equation for the particles balance as well). It becomes clear that the minimum for the Morse potential related to the gas phase is vacant, and a vapor molecule with low energy can be settled there, finishing in this way the very surface layer. This minimum lies in a space inside the gas phase but not inside the layer mentioned. The surface layer lies in the area of potential energy of the intermolecular interaction maximum. However, a softly condensed molecule, when getting in the minimum, imbeds anyway into the surface layer, sooner or later, without getting additional energy.As a result, quasi crystal phase presence and low kinetic energy of its vibrating molecules cause soft condensation instead of evaporation. The energy of the softly condensed  molecules redistributes at once by vibrating molecules of the quasi crystal area, and it is much more harder for them to quit the surface of the liquid; it is easier and more favorably to embed into it.The second above-mentioned condensation process is the condensation of those vapor molecules, whose one-particle kinetic energy is greater than or equal to the value ofL (see (5)). This energy is high enough for getting over the potential barrier formed by the molecules vibrating on the surface of the liquid. The number H of these “quick” vapor molecules penetrating into the volume of the liquid phase under study (per unit time and through a unit area of its surface) is defined by the equation below [1]:
(9)H=γ(kT2πm)1/2exp(-LkT)=γ(kT2πm)1/2exp(-æσV2/3T),
where æ(æ=l/k) may depend on T and on the nature of the investigated liquid phase (the coefficient l is explained before, relative to (5)). The condensation of such “quick” molecules may be called as “hard” condensation.Thus, just the vibrating molecules that form the surface layer of any liquid can cause the two above-considered condensation processes:(1) condensation of molecules, whose energy is less than or equal to E; (2) condensation of those molecules, whose energy is greater than or equal to L. For molecules with their one-particle kinetic energy ranging from E up to L, the surface layer of the liquid phase is an elastic interfacial molecular film, which reflects the given molecules back into the saturated vapor phase.For the saturated vapor phase, which is in equilibrium state with the corresponding liquid phase, the numberC must be equal to the sum of numbers D and H. In this way, we have from (7)–(9) (after cancelling their common multiplier (kT/2πm)1/2) the following equality:
(10)(zNaV)exp(-æσV2/3T)=γ(1-z+exp(-æσV2/3T)).Next, if it has been supposed that the saturated vapor phase obeys the perfect gas law, then the concentrationγ can be expressed by means of the following equation:
(11)γ=PkT,
where P is the saturated vapor pressure [1]. From (10) and (11) one can easily obtain the following expression used to calculate values of P:
(12)P=(zRV)exp(-æσV2/3T)[1-z+exp(-æσV2/3T)]-1,
where R(R=kNa) is the gas constant (R=8.3144 Jmol−1 K−1), and z is being defined by means of (4). In order to use (12) in practice, we should define the dependence of the quantity æ on T and the nature of the investigated liquid phase.


## 2.1. Method of Calculations Evaporation in Nonassociated Liquid

In order to find the above equation, let us consider one mole of a liquid with conformationally rigid molecules. Hereinafter we suppose that the given liquid is in thermal equilibrium with its saturated vapor (its temperatureT is within the interval between its normal freezing and normal boiling points). We shall consider all the molecules of the investigated liquid as spherical particles (hard spheres) due to their fast mutual reorientations. The above value of T is supposed to be high enough for the consideration to be valid.Here it is to be noted that the share of the evaporating molecules of this liquid is less than that of the molecules jumping within its volume. It has been shown [6] that the surface layer of any nonassociated liquid is formed of its vibrating molecules.Here, vibrating molecules are molecules of liquids with weight centres staying for a while in their potential wells formed by neighbouring molecules. Vibrating molecules may become jumping ones andvice versa, but they have also a period of “settled life,” which allows for considering them as vibrating molecules.Thus, molecules abandoning the liquid phase must have high enough values of their one-particle kinetic energy in order to get over the potential barrierL caused by the vibrating molecules belonging to the surface layer. As far as the energy well of a vibrating molecule is proportional to σV2/3 (see (3)), hereinafter we shall consider that the quantity L may be described by means of the following equation:
(5)L=lσV2/3.Equation (5) is similar to (3); however, there is a principal difference between them. The coefficient l in (5) may depend on T and on the nature of the investigated liquid phase as well. In other words, the quantity L is proportional to the energy of the one-particle potential well and also may depend on the structure of the surface layer, namely, its thickness which is being defined by the chemical nature of its vibrating molecules and the value of T of the given liquid phase. If one-particle kinetic energy of a jumping molecule is higher than the above mentioned its critical value L, the molecule will be capable of escaping liquid phase. The relative share s of such molecules may be found by means of the Boltzmann statistics [1]:
(6)s=exp(-LkT)=exp(-æσV2/3T),
where æ(æ=l/k), in its turn, depends on T and the nature of the liquid phase.For different non-associated liquids it was shown [6] that molecules in their near-surface layers form a peculiar quasi crystal phase. This phase is being formed for the account of jumping molecules quitting the near-surface layers when passing to the gas phase. By this, the temperature of these layers becomes lower than that in the whole volume of the liquid.The molecules of near-surface layers participate mainly in vibrational but not in jumping motion. Only they are responsible, from one part, for the surface tension phenomena in such liquids, and from the other part, namely, they form a potential barrier for evaporating or condensing molecules. The order in the given quasi crystal phase grows while nearing the surface layer of the liquid. From the liquid part, this area is messy enough, and its border is diffusive. In this work we suppose that the volume concentration of molecules in this area is practically equal to their concentration in the whole volume.Now, let the total number of all jumping molecules be equal tozNa (Na is Avogadro’s number) and let their volume concentration in the given liquid phase be n=zNa/V. Then the number C of collisions (per unit time) among the above-mentioned jumping molecules with energies greater than or equal to L and the vibrating ones situated on some unit area of the surface layer may be defined from the equation below [1]:
(7)C=n(kT2πm)1/2exp(-LkT)=(zNaV)(kT2πm)1/2exp(-æσV2/3T),
where m is the molecular mass of one molecule and the quantity z is being defined by means of (4). At the same time, C will be also equal to the number of evaporating jumping molecules, which are capable of quitting the investigated liquid through its unit surface per unit time (because their energy is high enough for getting over the surface layer).


## 2.2. Describing Condensation in Nonassociated Liquids

Now let us consider the inverse process of molecular condensation as passing from the saturated vapor phase into the considered liquid one. Hereinafter we shall suppose that the process can be divided into two simultaneous processes. The first one is the condensation of those vapor molecules, whose one-particle kinetic energy is less than or equal to the above-mentioned critical energyE (see (3)). In this case, attractive forces between vapour molecules and vibrating surface molecules are capable of fixing the former ones on the surface of the liquid. The number D of the vapor molecules that are being fixed on the area unit of this surface per unit time may be easily found by means of the following equation [1]:
(8)D=γ(kT2πm)1/2[1-exp(-EkT)]=γ(kT2πm)1/2(1-z),
where γ is the value of the total volume’s concentration for the molecules of the liquid under study in its saturated vapor phase. As far as for the considered fixed vapor molecules the critical value of one-particle kinetic energy E is being defined by (3); our (8) contains z as its parameter (see (4)). However, it should be noted that in (8) z denotes the relative share of those vapor molecules which can be fixed on the liquid surface due to the intermolecular attractive forces. The condensation of such “slow” molecules may be called as “soft” condensation.The presence of quasi-crystal area consisting of a few surface layers of the liquid (see [6]) is the reason of the fact that molecules moving to the surface layer (from either gas phase or liquid phase) must necessarily be influenced by a potential that has been formed by the molecules of the quasi-crystal area. This potential (from both sides of the very surface layer) will look like a Morse curve. However, the Morse curve, be it nearby the layer or in departure of it, can be represented by two parabolas, one for the area of minimum and the other for the more distant area. Thus, the energy of the quitting the surface level molecules will be described by two squared members being kinetic and potential energies of their interaction with quasi crystal molecules. According to the introduced approximation, potential energy of a molecule will quadratically depend on its distance till the very surface layer.In this way, square roots will appear nowhere (including the equation for the particles balance as well). It becomes clear that the minimum for the Morse potential related to the gas phase is vacant, and a vapor molecule with low energy can be settled there, finishing in this way the very surface layer. This minimum lies in a space inside the gas phase but not inside the layer mentioned. The surface layer lies in the area of potential energy of the intermolecular interaction maximum. However, a softly condensed molecule, when getting in the minimum, imbeds anyway into the surface layer, sooner or later, without getting additional energy.As a result, quasi crystal phase presence and low kinetic energy of its vibrating molecules cause soft condensation instead of evaporation. The energy of the softly condensed  molecules redistributes at once by vibrating molecules of the quasi crystal area, and it is much more harder for them to quit the surface of the liquid; it is easier and more favorably to embed into it.The second above-mentioned condensation process is the condensation of those vapor molecules, whose one-particle kinetic energy is greater than or equal to the value ofL (see (5)). This energy is high enough for getting over the potential barrier formed by the molecules vibrating on the surface of the liquid. The number H of these “quick” vapor molecules penetrating into the volume of the liquid phase under study (per unit time and through a unit area of its surface) is defined by the equation below [1]:
(9)H=γ(kT2πm)1/2exp(-LkT)=γ(kT2πm)1/2exp(-æσV2/3T),
where æ(æ=l/k) may depend on T and on the nature of the investigated liquid phase (the coefficient l is explained before, relative to (5)). The condensation of such “quick” molecules may be called as “hard” condensation.Thus, just the vibrating molecules that form the surface layer of any liquid can cause the two above-considered condensation processes:(1) condensation of molecules, whose energy is less than or equal to E; (2) condensation of those molecules, whose energy is greater than or equal to L. For molecules with their one-particle kinetic energy ranging from E up to L, the surface layer of the liquid phase is an elastic interfacial molecular film, which reflects the given molecules back into the saturated vapor phase.For the saturated vapor phase, which is in equilibrium state with the corresponding liquid phase, the numberC must be equal to the sum of numbers D and H. In this way, we have from (7)–(9) (after cancelling their common multiplier (kT/2πm)1/2) the following equality:
(10)(zNaV)exp(-æσV2/3T)=γ(1-z+exp(-æσV2/3T)).Next, if it has been supposed that the saturated vapor phase obeys the perfect gas law, then the concentrationγ can be expressed by means of the following equation:
(11)γ=PkT,
where P is the saturated vapor pressure [1]. From (10) and (11) one can easily obtain the following expression used to calculate values of P:
(12)P=(zRV)exp(-æσV2/3T)[1-z+exp(-æσV2/3T)]-1,
where R(R=kNa) is the gas constant (R=8.3144 Jmol−1 K−1), and z is being defined by means of (4). In order to use (12) in practice, we should define the dependence of the quantity æ on T and the nature of the investigated liquid phase.


## 3. Results and Discussion

### 3.1. Definition of the Temperature Dependence ofæ

To define the dependence ofæ on T, let us consider the compounds presented in Table 1. (Here it should be reminded that we consider liquids, whose molecules are conformationally rigid.)Table 1
To the definition of the temperature dependence ofæ.
No.
Compound
σ
×
1
0
3 (N m−1)
V
×
1
0
6 (m3 mol−1)
T (K)
T
c (K)
P (Pa)
τ
æ × 10−7 (J−1 K mol2/3)
ξ
×
1
0
-
7 (J−1 K mol2/3)
1
Fluorine
19.07
23.48
65.00
144.3
4719
0.4505
2.6407
5.8617
13.42
25.17
85.20
101325
0.5904
3.4600
5.8604
2
Silane
16.17
51.85
153.15
269.6
62104
0.5681
3.3305
5.8625
15.11
52.77
161.30
101325
0.5983
3.5082
5.8636
3
Carbontetrachloride
24.60
98.76
311.45
556.4
26795
0.5598
3.2795
5.8583
20.42
103.91
349.95
101325
0.6290
3.6904
5.8671Experimental values ofσ, V, and P for all these compounds that participate in the calculation of æ are taken from [3, 7–11]. The comparison of numerical values of æ calculated with their use in (12) shows that for all compounds from Table 1  æ is directly proportional to τ, where τ(τ=T/Tc) denotes the reduced temperature of the compounds. Hereinafter Tc denotes critical temperatures of investigated liquids. For the liquids presented in Table 1 their values of Tc were taken from [7]. The data in the last column of Table 1 show that the ratio ξ(ξ=æ/τ) remains constant and does not depend on T and the nature of the liquid under study. Thus, the expression for the quantity æ entering (12) looks like
(13)æ=ξTTc.Then (12) will have the form
(14)P=(zRTV)exp(-ξσV2/3Tc)[1-z+exp(-ξσV2/3Tc)]-1.Here it is worth to be noted that the value ofz in (14) has been defined by means of (4) with the symbol T (but not Tc) in the name of the exponent.


### 3.2. Towards the Evaluation of the Constantξ

In order to verify (13) and (14) and to define the quantity ξ more exactly, the compounds presented in Table 2 were investigated. Experimental values of σ, V, Tc, and P were taken from [3, 7–13].Table 2
Towards the evaluation of the constantξ.
No.
Compound
σ
×
1
0
3 (N m−1)
V
×
1
0
6 (m3 mol−1)
T (K)
T
c (K)
P (Pa)
ξ
1
Nitrogen
8.88
34.73
77.35
126.2
101325
5.9176
2
Carbon monoxide
9.58
34.88
81.00
132.9
93599
5.8474
3
Oxygen
13.20
28.07
90.19
154.35
101325
5.8607
4
Methane
15.36
36.17
100.00
190.85
34000
5.8752
5
Ethylene
18.56
48.05
158.46
282.4
50446
5.8838
6
Trifluorochloromethane
18.37
63.40
163.15
301.9
16140
5.9117
7
Perchloryl fluoride
20.12
59.5
223.15
368.4
89346
5.8673
8
Iodomethane
29.72
63.1
303.15
528
65143
5.8570
9
Carbon disulfide
31.85
61.0
303.15
552
57943
5.9133
10
Arsenic tribromide
29.10
109.1
494.0
785
101325
5.8899The data in Table2 show that ξ does remain constant for these compounds, although their chemical structures differ significantly. The average numerical value of the constant ξ defined from the data sets in Tables 1 and 2 is equal to 5.8748×107 (J−1 K mol−2/3).Now let us consider the case when our molecules haveN energetically degenerated (or quasi-degenerated) conformational states in the liquid phase. It has been shown [14] that the intramolecular conformational transitions occurring among these states will lead to the corresponding increase in the total number of bimolecular collisions between neighboring molecules. This increase can be described (see [14]) by means of the function G(N), whose analytical form is
(15)G(N)=(1-θlnN)-1.In (15) its dimensionless constant θ does not depend on T and the nature of the liquid phase. It is equal to 0.05681 [14]. (For liquids with conformationally rigid molecules N=1 and G(1)=1.)Now let us consider the process of piercing of the evaporating conformationally flexible “hot” molecules through the vibrating molecules of the surface layer. Hereinafter we shall suppose that these vibrating molecules are fixed in one of their conformational states, due to the action of the attractive force field existing between them and also due to the above-mentioned absence of the translational jumping motion for the molecules of the surface layer [6]. In other words, it is presupposed that the presence of uncompensated attractive force (the latter causes the surface tension in the investigated liquid and is directed into its volume) leads to the fixation of each molecule of the surface layer in one of its conformations. Thus, the evaporating “hot” molecules, which are capable of making transitions among their conformational states, will pierce the surface layer formed by the vibrating molecules existing in only one conformational state.


### 3.3. Evaporating Conformationally Flexible Molecules

Further, let us consider interaction of two neighboring molecules of the liquid under study. If each of these molecules can haveN conformational states, then the increase in the number of their bimolecular collisions is being described by means of the function G(N) (see (15)). Now let us imagine that for one of these molecules (hereinafter, the first molecule) its conformational transitions are stopped (i.e., the molecule is fixed in one of its conformations). In this case, the increase I˙ in the number of bimolecular collisions between the considered molecules will be caused by conformational transitions of the second (conformationally flexible) molecule. As the situation under consideration is symmetrically reversible with respect to both molecules (namely, the first molecule is considered as conformationally flexible and the second one is conformationally rigid), so the above increase I˙ is to be equal to the square root of the function G(N):
(16)I˙=[G(N)]1/2.And in the case, when both neighboring molecules interact while doing their conformational transitions, the total increase in the number of their bimolecular collisions will be equal toI˙2 (and, therefore, to G(N)).When the evaporating molecules of the liquid phase pierce through the vibrating molecules of its surface layer, we have the realization of the above-considered situation in practice. Thinking the evaporating molecules as piercing the surface layer, we deal with the translational motion of a conformationally flexible molecule through the layer of conformationally rigid ones. Hereafter we shall consider that the one-particle potential barrierL (see (5)) which must be got over by this molecule is also proportional to the number of its bimolecular collisions with the corresponding molecules of the surface layer. Thus, in order to calculate the barrier L adequately, we must take into account the increase in the number of the bimolecular collisions which are caused by the conformational transitions of this evaporating molecule. Bearing in mind the above-mentioned reasons related to the quantity I˙ describing this increase (see (16)), we can rewrite (5) in the following form:
(17)L=[G(N)]1/2lσV2/3.Thus, for the saturated vapor pressureP of those liquids, whose molecules can have their conformational transitions, the following final expression holds:
(18)P=(zRTV)exp(-ξ[G(N)]1/2σV2/3Tc)×[1-z+exp(-ξ[G(N)]1/2σV2/3Tc)]-1.In order to verify (18) let us therein denote the product ξ[G(N)]1/2 as ω. The values of ω calculated on the basis of (18) are presented in Table 3 for the liquids, whose molecules have conformational transitions.Table 3
To the definition of the dependence ofω on N.
No.
Compound
N
σ
×
1
0
3 (N m−1)
V
×
1
0
6 (m3 mol−1)
T (K)
T
c (K)
P (Pa)
ω
ω
/
[
G
(
N
)
]
1
/
2
1
Ethane
3
18.47
53.49
170.00
305.4
42940
6.1065
5.9129
2
Trimethylamine
2
×
3
3
16.24
88.11
273.15
433.2
90271
6.6650
5.8614
3
1,4-Dioxane
4
27.88
89.3
333.15
587
23803
6.1551
5.9078Experimental values ofσ, V, Tc, and P required for the calculation of ω were taken from [3, 7, 8, 10, 15]. Here the definition of N (the number of one-particle conformational states for the molecules of the investigated liquids) is to be mentioned. For any such molecule, the value of N in (15) and (18) is supposed to be equal to the total number of local minima on the surface of its full internal potential energy, which arise on this surface under all possible internal rotations and intramolecular inversions that change the conformation of its skeleton [5, 16]. All its atoms are considered hereinafter as non-equivalent. Thus, in the case of ethane (see Table 3) its molecule may pass through three its possible (hindered) conformations, which arise from the internal rotations around C–C bond.In the case of trimethylamine, the internal rotation around each of its C–N bonds can be characterized by the presence of three local minima on the surface of its internal one-particle potential energy [17]. As the one-particle number of the above C–N bonds is equal to three, so the number of the minima connected with three internal C–N rotations will be 33. For the molecule of trimethylamine we have also to take into account the spatial inversion of its nitrogen atom [17]. The given type of internal one-particle motion leads to the total number of the above mentioned minima equal to 2×33.1,4-Dioxane may have intra-molecular conformational transitions among four its possible conformations: two conformations of the type “chair” and two conformations of the type “bath” [17]. So, for 1,4-dioxane N=4. The usage of the above considered values of N for the calculation of the ratio ω/[G(N)]1/2 shows (see Table 3) that this ratio is the constant ξ found above (cf. the data of Tables 2 and 3).Thus, bearing in mind thatG(1)=1, we can use (18) for the calculations of the quantity P for various nonassociated liquids formed by both conformationally rigid and conformationally flexible molecules.


### 3.4. The Calculation of the Quantity Vapor Pressure of the Inorganic and Organic Liquids

The values of the saturated vapor pressure of the inorganic and organic liquids presented in Table4 were calculated by means of (18). Experimental values of σ, V, Tc needed for this calculation were taken from [1, 3, 7–11, 15] and also from [18–27]. The values of N were calculated on the base of data presented in [17, 28]. Note that in the case of the benzene derivatives (see Table 4) the internal rotation around any of their C–C bonds (where one of carbon atoms belongs to the benzene ring) corresponds to six local minima of their one-particle potential energy [17].Table 4
The calculation of the quantityP by means of (18).
No.
Compound
N
σ
×
1
0
3 (N m−1)
V
×
1
0
6 (m3 mol−1)
T (K)
T
c (K)
P (Pa)
Calc.
Exper.
1
2
3
4
5
6
7
8
9
1
Argon*
1
13.3912.62
27.9728.49
83.8187.29
150.8
68053101231
68750101325
2
Krypton
1
16.40
34.17
115.76
209.4
72281
72920
3
Xenon
1
19.30
43.34
161.36
289.7
82319
81627
4
Diborane
1
16.49
61.92
163.15
290
34422
34062
5
Chlorine
1
35.69
42.68
201.45
417.0
12845
13332
6
Difluorodichloromethane
1
18.81
78.10
223.15
385.2
38763
39330
7
Bromine
1
44.10
50.90
286.15
584
16887
16799
8
Titanium tetrabromide
1
29.68
138.9
433.15
795.6
15814
15720
9
Mercury(II) bromide
1
58.30
72.1
549.15
1011
36193
37732
10
Propane
32
19.20
71.83
203.15
369.8
23212
24312
11
Dimethyl sulfide
32
24.46
73.27
293.15
503.0
53910
53033
12
Bromoethane
3
24.90
74.89
293.15
503.8
50635
51436
13
Cyclopentene
2
22.65
88.23
293.15
506.0
42258
41621
14
1,2-Dichloroethane
3
25.40
83.7
343.15
561
63965
64631
15
Toluene
6
22.90
112.8
343.15
591.7
28256
27164
16
o-Xylene
62
24.32
127.7
343.15
632.2
8301
8426
17
m-Xylene
62
23.16
129.1
343.15
619.2
10199
10121
18
p-Xylene
62
22.86
130.0
343.15
616.2
10533
10501
19
Ethylbenzene
3
×
6
23.39
129.1
343.15
619.6
10970
11296
20
1,2-Dichloropropane
32
21.50
105.1
353.15
577
59250
60704
21
Sulfur monochloride
2
29.10
89.63
393.15
665
63171
62822
22
1,3,5-Trimethyl-benzene
63
15.01
163.0
437.9
642.1
100882
101325
23
Naphthalene
1
22.10
146.5
491.1
748.4
100010
101325
*The quantity P for argon was calculated at its triple point and at its normal boiling one.Thus, for instance, the total numberN of 1,3,5-trimethylbenzene will be 63. The comparison of the calculated values of P and the experimental ones taken from [3, 8, 9, 15, 21, 23] shows that (18) describes the quantity P adequately. The average absolute value (module) of calculation error for P is 1.6% (Table 4).However, such low-boiling quantum liquids as helium and hydrogen do not obey (18). This equation does not feet also for liquid metals, ionic liquids, and the chemical compounds, whose molecules are strongly associated in their liquid phase: water, alcohols, and so on. Thus, for instance, for quinoline being the associated liquid (and considered at its normal boiling point—510.85 K [15]), experimental values of σ, V, and Tc are equal to 23.23×10-3 (Nm−1), 142.0×10-6 (m3 mol−1), and 782.2 K, respectively [15, 29, 30]. The value of P calculated by means of (18) equals 117305 Pa (instead of 101325 Pa). At the same time, naphthalene, whose molecules are nonpolar, obeys (18) at its normal boiling point (see Table 4).


## 3.1. Definition of the Temperature Dependence ofæ

To define the dependence ofæ on T, let us consider the compounds presented in Table 1. (Here it should be reminded that we consider liquids, whose molecules are conformationally rigid.)Table 1
To the definition of the temperature dependence ofæ.
No.
Compound
σ
×
1
0
3 (N m−1)
V
×
1
0
6 (m3 mol−1)
T (K)
T
c (K)
P (Pa)
τ
æ × 10−7 (J−1 K mol2/3)
ξ
×
1
0
-
7 (J−1 K mol2/3)
1
Fluorine
19.07
23.48
65.00
144.3
4719
0.4505
2.6407
5.8617
13.42
25.17
85.20
101325
0.5904
3.4600
5.8604
2
Silane
16.17
51.85
153.15
269.6
62104
0.5681
3.3305
5.8625
15.11
52.77
161.30
101325
0.5983
3.5082
5.8636
3
Carbontetrachloride
24.60
98.76
311.45
556.4
26795
0.5598
3.2795
5.8583
20.42
103.91
349.95
101325
0.6290
3.6904
5.8671Experimental values ofσ, V, and P for all these compounds that participate in the calculation of æ are taken from [3, 7–11]. The comparison of numerical values of æ calculated with their use in (12) shows that for all compounds from Table 1  æ is directly proportional to τ, where τ(τ=T/Tc) denotes the reduced temperature of the compounds. Hereinafter Tc denotes critical temperatures of investigated liquids. For the liquids presented in Table 1 their values of Tc were taken from [7]. The data in the last column of Table 1 show that the ratio ξ(ξ=æ/τ) remains constant and does not depend on T and the nature of the liquid under study. Thus, the expression for the quantity æ entering (12) looks like
(13)æ=ξTTc.Then (12) will have the form
(14)P=(zRTV)exp(-ξσV2/3Tc)[1-z+exp(-ξσV2/3Tc)]-1.Here it is worth to be noted that the value ofz in (14) has been defined by means of (4) with the symbol T (but not Tc) in the name of the exponent.


## 3.2. Towards the Evaluation of the Constantξ

In order to verify (13) and (14) and to define the quantity ξ more exactly, the compounds presented in Table 2 were investigated. Experimental values of σ, V, Tc, and P were taken from [3, 7–13].Table 2
Towards the evaluation of the constantξ.
No.
Compound
σ
×
1
0
3 (N m−1)
V
×
1
0
6 (m3 mol−1)
T (K)
T
c (K)
P (Pa)
ξ
1
Nitrogen
8.88
34.73
77.35
126.2
101325
5.9176
2
Carbon monoxide
9.58
34.88
81.00
132.9
93599
5.8474
3
Oxygen
13.20
28.07
90.19
154.35
101325
5.8607
4
Methane
15.36
36.17
100.00
190.85
34000
5.8752
5
Ethylene
18.56
48.05
158.46
282.4
50446
5.8838
6
Trifluorochloromethane
18.37
63.40
163.15
301.9
16140
5.9117
7
Perchloryl fluoride
20.12
59.5
223.15
368.4
89346
5.8673
8
Iodomethane
29.72
63.1
303.15
528
65143
5.8570
9
Carbon disulfide
31.85
61.0
303.15
552
57943
5.9133
10
Arsenic tribromide
29.10
109.1
494.0
785
101325
5.8899The data in Table2 show that ξ does remain constant for these compounds, although their chemical structures differ significantly. The average numerical value of the constant ξ defined from the data sets in Tables 1 and 2 is equal to 5.8748×107 (J−1 K mol−2/3).Now let us consider the case when our molecules haveN energetically degenerated (or quasi-degenerated) conformational states in the liquid phase. It has been shown [14] that the intramolecular conformational transitions occurring among these states will lead to the corresponding increase in the total number of bimolecular collisions between neighboring molecules. This increase can be described (see [14]) by means of the function G(N), whose analytical form is
(15)G(N)=(1-θlnN)-1.In (15) its dimensionless constant θ does not depend on T and the nature of the liquid phase. It is equal to 0.05681 [14]. (For liquids with conformationally rigid molecules N=1 and G(1)=1.)Now let us consider the process of piercing of the evaporating conformationally flexible “hot” molecules through the vibrating molecules of the surface layer. Hereinafter we shall suppose that these vibrating molecules are fixed in one of their conformational states, due to the action of the attractive force field existing between them and also due to the above-mentioned absence of the translational jumping motion for the molecules of the surface layer [6]. In other words, it is presupposed that the presence of uncompensated attractive force (the latter causes the surface tension in the investigated liquid and is directed into its volume) leads to the fixation of each molecule of the surface layer in one of its conformations. Thus, the evaporating “hot” molecules, which are capable of making transitions among their conformational states, will pierce the surface layer formed by the vibrating molecules existing in only one conformational state.


## 3.3. Evaporating Conformationally Flexible Molecules

Further, let us consider interaction of two neighboring molecules of the liquid under study. If each of these molecules can haveN conformational states, then the increase in the number of their bimolecular collisions is being described by means of the function G(N) (see (15)). Now let us imagine that for one of these molecules (hereinafter, the first molecule) its conformational transitions are stopped (i.e., the molecule is fixed in one of its conformations). In this case, the increase I˙ in the number of bimolecular collisions between the considered molecules will be caused by conformational transitions of the second (conformationally flexible) molecule. As the situation under consideration is symmetrically reversible with respect to both molecules (namely, the first molecule is considered as conformationally flexible and the second one is conformationally rigid), so the above increase I˙ is to be equal to the square root of the function G(N):
(16)I˙=[G(N)]1/2.And in the case, when both neighboring molecules interact while doing their conformational transitions, the total increase in the number of their bimolecular collisions will be equal toI˙2 (and, therefore, to G(N)).When the evaporating molecules of the liquid phase pierce through the vibrating molecules of its surface layer, we have the realization of the above-considered situation in practice. Thinking the evaporating molecules as piercing the surface layer, we deal with the translational motion of a conformationally flexible molecule through the layer of conformationally rigid ones. Hereafter we shall consider that the one-particle potential barrierL (see (5)) which must be got over by this molecule is also proportional to the number of its bimolecular collisions with the corresponding molecules of the surface layer. Thus, in order to calculate the barrier L adequately, we must take into account the increase in the number of the bimolecular collisions which are caused by the conformational transitions of this evaporating molecule. Bearing in mind the above-mentioned reasons related to the quantity I˙ describing this increase (see (16)), we can rewrite (5) in the following form:
(17)L=[G(N)]1/2lσV2/3.Thus, for the saturated vapor pressureP of those liquids, whose molecules can have their conformational transitions, the following final expression holds:
(18)P=(zRTV)exp(-ξ[G(N)]1/2σV2/3Tc)×[1-z+exp(-ξ[G(N)]1/2σV2/3Tc)]-1.In order to verify (18) let us therein denote the product ξ[G(N)]1/2 as ω. The values of ω calculated on the basis of (18) are presented in Table 3 for the liquids, whose molecules have conformational transitions.Table 3
To the definition of the dependence ofω on N.
No.
Compound
N
σ
×
1
0
3 (N m−1)
V
×
1
0
6 (m3 mol−1)
T (K)
T
c (K)
P (Pa)
ω
ω
/
[
G
(
N
)
]
1
/
2
1
Ethane
3
18.47
53.49
170.00
305.4
42940
6.1065
5.9129
2
Trimethylamine
2
×
3
3
16.24
88.11
273.15
433.2
90271
6.6650
5.8614
3
1,4-Dioxane
4
27.88
89.3
333.15
587
23803
6.1551
5.9078Experimental values ofσ, V, Tc, and P required for the calculation of ω were taken from [3, 7, 8, 10, 15]. Here the definition of N (the number of one-particle conformational states for the molecules of the investigated liquids) is to be mentioned. For any such molecule, the value of N in (15) and (18) is supposed to be equal to the total number of local minima on the surface of its full internal potential energy, which arise on this surface under all possible internal rotations and intramolecular inversions that change the conformation of its skeleton [5, 16]. All its atoms are considered hereinafter as non-equivalent. Thus, in the case of ethane (see Table 3) its molecule may pass through three its possible (hindered) conformations, which arise from the internal rotations around C–C bond.In the case of trimethylamine, the internal rotation around each of its C–N bonds can be characterized by the presence of three local minima on the surface of its internal one-particle potential energy [17]. As the one-particle number of the above C–N bonds is equal to three, so the number of the minima connected with three internal C–N rotations will be 33. For the molecule of trimethylamine we have also to take into account the spatial inversion of its nitrogen atom [17]. The given type of internal one-particle motion leads to the total number of the above mentioned minima equal to 2×33.1,4-Dioxane may have intra-molecular conformational transitions among four its possible conformations: two conformations of the type “chair” and two conformations of the type “bath” [17]. So, for 1,4-dioxane N=4. The usage of the above considered values of N for the calculation of the ratio ω/[G(N)]1/2 shows (see Table 3) that this ratio is the constant ξ found above (cf. the data of Tables 2 and 3).Thus, bearing in mind thatG(1)=1, we can use (18) for the calculations of the quantity P for various nonassociated liquids formed by both conformationally rigid and conformationally flexible molecules.


## 3.4. The Calculation of the Quantity Vapor Pressure of the Inorganic and Organic Liquids

The values of the saturated vapor pressure of the inorganic and organic liquids presented in Table4 were calculated by means of (18). Experimental values of σ, V, Tc needed for this calculation were taken from [1, 3, 7–11, 15] and also from [18–27]. The values of N were calculated on the base of data presented in [17, 28]. Note that in the case of the benzene derivatives (see Table 4) the internal rotation around any of their C–C bonds (where one of carbon atoms belongs to the benzene ring) corresponds to six local minima of their one-particle potential energy [17].Table 4
The calculation of the quantityP by means of (18).
No.
Compound
N
σ
×
1
0
3 (N m−1)
V
×
1
0
6 (m3 mol−1)
T (K)
T
c (K)
P (Pa)
Calc.
Exper.
1
2
3
4
5
6
7
8
9
1
Argon*
1
13.3912.62
27.9728.49
83.8187.29
150.8
68053101231
68750101325
2
Krypton
1
16.40
34.17
115.76
209.4
72281
72920
3
Xenon
1
19.30
43.34
161.36
289.7
82319
81627
4
Diborane
1
16.49
61.92
163.15
290
34422
34062
5
Chlorine
1
35.69
42.68
201.45
417.0
12845
13332
6
Difluorodichloromethane
1
18.81
78.10
223.15
385.2
38763
39330
7
Bromine
1
44.10
50.90
286.15
584
16887
16799
8
Titanium tetrabromide
1
29.68
138.9
433.15
795.6
15814
15720
9
Mercury(II) bromide
1
58.30
72.1
549.15
1011
36193
37732
10
Propane
32
19.20
71.83
203.15
369.8
23212
24312
11
Dimethyl sulfide
32
24.46
73.27
293.15
503.0
53910
53033
12
Bromoethane
3
24.90
74.89
293.15
503.8
50635
51436
13
Cyclopentene
2
22.65
88.23
293.15
506.0
42258
41621
14
1,2-Dichloroethane
3
25.40
83.7
343.15
561
63965
64631
15
Toluene
6
22.90
112.8
343.15
591.7
28256
27164
16
o-Xylene
62
24.32
127.7
343.15
632.2
8301
8426
17
m-Xylene
62
23.16
129.1
343.15
619.2
10199
10121
18
p-Xylene
62
22.86
130.0
343.15
616.2
10533
10501
19
Ethylbenzene
3
×
6
23.39
129.1
343.15
619.6
10970
11296
20
1,2-Dichloropropane
32
21.50
105.1
353.15
577
59250
60704
21
Sulfur monochloride
2
29.10
89.63
393.15
665
63171
62822
22
1,3,5-Trimethyl-benzene
63
15.01
163.0
437.9
642.1
100882
101325
23
Naphthalene
1
22.10
146.5
491.1
748.4
100010
101325
*The quantity P for argon was calculated at its triple point and at its normal boiling one.Thus, for instance, the total numberN of 1,3,5-trimethylbenzene will be 63. The comparison of the calculated values of P and the experimental ones taken from [3, 8, 9, 15, 21, 23] shows that (18) describes the quantity P adequately. The average absolute value (module) of calculation error for P is 1.6% (Table 4).However, such low-boiling quantum liquids as helium and hydrogen do not obey (18). This equation does not feet also for liquid metals, ionic liquids, and the chemical compounds, whose molecules are strongly associated in their liquid phase: water, alcohols, and so on. Thus, for instance, for quinoline being the associated liquid (and considered at its normal boiling point—510.85 K [15]), experimental values of σ, V, and Tc are equal to 23.23×10-3 (Nm−1), 142.0×10-6 (m3 mol−1), and 782.2 K, respectively [15, 29, 30]. The value of P calculated by means of (18) equals 117305 Pa (instead of 101325 Pa). At the same time, naphthalene, whose molecules are nonpolar, obeys (18) at its normal boiling point (see Table 4).


## 4. Conclusion

The following conclusions may be drawn. Equation (18) allows us to perform the calculation of the saturated vapor pressure for various nonassociated liquids. There are two types of the condensation process of the nonassociated liquids: soft and hard molecular condensation. For a part of vapor molecules their surface layer behaves as some impenetrable elastic film. For the evaporating conformationally flexible molecules their one-particle potential barrier caused by the vibrating surface molecules is essentially higher than that for the evaporating conformationally rigid ones. The increase in the value of this barrier can be properly described by means of (17).



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*Source: 964091-2013-12-28.xml*