In his classic treatise [1] , Gibbs introduced the concept of a state function of any two state variables, for example pressure (p) as a function of temperature (T) and volume (V) as illustrated in Figure 1 p-V-T 3D phase diagram. Given the state function heat capacity at constant pressure (C_p), Gibbs defined both enthalpy (dU + pdV = C_pdT) and entropy (dS = C_pdlog_eT), that are precise statements of the 1^st- and 2^nd-laws of classical thermodynamics, respectively [3] .

Every thermodynamic state point on a Gibbs surface is defined where two lines cross and characterised by the number of degrees of freedom (F) in its specification by Gibbs phase rule. For a one-component system (C = 1) then, for P phases in coexistence, F = C − P + 2. All single-phase state points when (F = 2) are defined when an isotherm crosses an isobar, i.e., by T, p. A state point in a two-phase region (F = 1) is defined when either an isotherm or an isobar crosses a coexistence line. The coexistence lines are defined by the intersection of lines of chemical potential (μ), on the μ(p,T) surface. The triple point volumes (Figure 1) are defined by the intersection of two coexistence lines. There is no such consistent thermodynamic definition of the “critical point”, shown in Figure 1.

van der Waals assumed that the cubic Equation-of-state

p = ρ k T 1 − b ρ − a ρ 2 (1)

has a singularity that confirms the existence of a critical volume to be an established scientific truth. The van der Waals interpretation, also depicted as p-T phase diagram in Figure 2, was based upon just two near-critical isotherms with limited p(V,T) data points for CO₂ reported in 1869 by Andrews. The Andrews-van der Waals hypothesis gave rise to the earliest predictions of solid-liquid-gas phase diagrams.

The Gibbs phase rule for all state points on the p-T surface gave rise to various conjectures of p-T diagrams showing gas, liquid, and solid regions. In the very early days, the solid-liquid transition was believed to be independent of pressure, and the gas-liquid coexistence line was reasonably known. Gibbs [4] , unaware of van der Waals’ thesis at the time also interpreted Andrews’ discovery of a temperature above which a gas could not be liquified by increasing pressure. Gibbs noted that there is also a pressure above which a gas cannot be liquified by reducing the temperature. Gibbs thought there was a second triple point and described the region as the “critical phase” as distinct from van der Waals continuous fluid hypothesis (Figure 3(a)). Hannay [5] also correctly observed that the Andrews experiments are indicative of a 1^st-order phase transition at T_c.

Figure 3(b) for CO₂, drawn from present NIST thermophysical fluid property data [6] , shows the definition and determination of the critical p, T point where the two percolation lines cross. The Gibbs-Hannay interpretation is closer to the modern description of the critical line between coexisting densities at T_c. The critical density hiatus and supercritical mesophase are now established science, confirmed by computer experiments on minimalist models [7] , confirmed by review in depth from the literature experimental measurements covering 150 years since Andrew’s [8] , and, recently confirmed, inter alia, by the debunked universality hypothesis [9] .

Gas and liquid percolation lines, PB and PA, are defined by a change in the state function rigidity (ω) when hetero-phase bonded clusters of “liquid” in gas (density ρ_PB) and clusters of “gas” in liquid (density ρ_PA) have the same T, p and G (Gibbs chemical potential) at two different coexisting densities. This condition defines a 1^st-order phase transition. At the gas-liquid critical point T_c-p_c the rigidity of both phases goes to zero, triggering a phase transition that terminates at the critical 2-phase coexistence pressure where the percolation lines intersect. Figure 2 and Figure 3 show that Gibbs and Hannay were closer to the scientific truth than van der Waals and the prevailing universality hypotheses of theoretical physics, and NIST employees still [6] [7] [8] [9] .

Rigidity is a defining state function that describes the distinction between gas states below the Boyle temperature and liquid or solid states. It decreases with density for a gas and increases with density for a liquid or solid. It is a reciprocal compressibility and related to Gibbs energy and hence also to density fluctuations by the following equalities of classical and statistical thermodynamics.

ω = ( d p d ρ ) T = − V K T = V ( d p d ln V ) T = ρ ( d G d p ) T = ( d μ d ln N ) V , T = R T / ( 〈 Δ N 2 〉 ) V , T (2)

where K_T is the isothermal compressibility, G is Gibbs energy, μ is Gibbs chemical potential and (N/V) is number density. It is the symmetry of the rigidity, rather than the compressibility, that reveals the connection to percolation transitions that can define the distinction between gaseous states, and liquid or solid states below the Boyle temperature. Accurate rigidity data have been used, inter alia, to invalidate hypotheses that describe all gas-liquid critical points as being a singularity with universal scaling laws [9] .

For pure fluids, rigidities can be obtained from the heat capacity data in NIST thermophysical web book [6] , given the speed of sound (c) values and the heat capacity ratio, then ω = c 2 C p / C v . The rigidities of isotherms below T_B are shown in Figure 4 for CO₂.

The Boyle-work (BW) line (w = p/ρ_BW = RT) [10] is seen to be perfectly linear for CO₂. A similar line can be defined by the rigidity symmetry (RS) line (ω = dp/dρ)_T = RT), defined as ρ_RS(T), connects all state density points on the isotherms at a somewhat lower density than ρ_BW(T) when the ω(ρ,T) state point has the same rigidity (ω) as the ideal gas at that temperature. The RS line is also linear. In the following sections we will relate the RS line to the BW line.

An inspection of the ω(T) isotherms in Figure 4 shows a symmetry that is consistent with the existence of a supercritical mesophase within which it

remains constant along any isotherm and decreases from RT at the Boyle temperature (T_B: defined as in Figure 4 as isotherm above which there is no minimum in p(ρ)_T), to zero within the critical divide for all fluids [7] [8] .

The percolation transition lines shown in Figure 4 are manifested as third- and higher-order discontinuities in the Gibbs energy p-T derivatives that depend upon density fluctuations. As the coexisting densities of liquid and gas densities become closer with T < T_c, the fluctuations increasingly reflect a symmetric hetero-phase presence in both phases. The experimental evidence for heterophase fluctuations is reproducible and well documented: see e.g., the review of Yukalov [11] . The role of heterophase fluctuations in gas-liquid criticality by percolation of the phase volume has been established. This implies changes of state in composition of the system, but still in-keeping with Gibbs definition of a “phase”, i.e., with two degrees of freedom, T and p as originally observed by Gibbs for “critical phases” [4] . The symmetry seen for CO₂ appears to be a characteristic property of all pure atomic and molecular liquids regardless of the Hamiltonian complexity, even for water.

The observations regarding CO₂ also apply to complex liquids, and in particular the critical coexistence properties for steam and water [12] . Notwithstanding the known complexities of the steam-water molecule, and the quantum effects of the H-bonds in cluster and solid structures, the thermodynamic Equation-of-state for water reveals a near perfect steam-water rigidity symmetry, and hence also a linear ρ_RS(T) line. The data, illustrated in Figure 5, can be obtained from NIST tabulations [6] which has been calculated from the Wagner-Pruss Equation-of-state [13] . For water, the NIST Equation-of-state [6] [13] contains upwards of 100 arbitrary adjustable parameters to represent the experimental thermophysical fluid data to within an accuracy that it has been measured.

Given the correct scientific description of the phase transitions, the percolation lines PB and PA, and the BW and RS lines, this number of adjustable parameters can be reduced to zero, without loss of precision, provided we can deduce the correct science to determine the necessary physical constants. We illustrate this plausible objective briefly here, with just one supercritical isotherm (673 K or 400˚C), and a point on the RS line (Figure 5) i.e. density ρ_rs = 35.5 mol/l corresponding to the rigidity ω = 5.65 kJ/mol of the ideal gas steam limit ρ → 0 .

From Figure 5 we infer the following:

1) The thermodynamic state functions, e.g. p(ρ,T), of steam along any isotherm below T_B, for all densities below the percolation transition density ρ_PB(T), will be continuous in all derivatives, and represented by a virial expansion in powers of density.

2) Given the rigidity symmetry seen in Figure 5, p(ρ,T) for water can be obtained from the same expansion coefficients used to describe steam isotherms at the higher densities above ρ_PA(T) and for densities below the RS line on any isotherm in an expansion in powers of the density difference Δρ_RS = (ρ − ρ_RS)_T.

3) The function p(ρ)_T and p(Δρ_RS)_T are empirically quadratic. If that is the

general case, the same two virial coefficients that describe the gas phase for densities below the PB line can be used to represent the p(ρ,T) data for the supercritical liquid region between T_c and T_B for densities between the PA and RS lines at, and above the PA line, i.e. ρ_PA(T).

4) The RS line shown has a pressure of 155 MPa at 673 K. The whole isotherm, experimentally, extends to higher temperatures, up to T_B (= 1250 K) for steam, and pressures to 1000 MPa [13] . This region is amenable to an expansion around the BW line ρ_BW(T) along the same isotherm.

5) The steam section, including the mesophase, requires only the first 2 or 3 coefficients in an expansion in powers of density, the two physical constant densities ρ_PB and ρ_PA, and the Boyle temperature T_B, for accurate representation of ω(T = 673), over the whole measured pressure range up to 1000 MPa of its existence for densities below and above ρ_PB and ρ_PA respectively.

6) The same coefficients that describe the steam density expansion could also describe an expansion about density point ρ_RS on the water phase in powers of the density difference Δρ = (ρ_RS − ρ)_water along the same isotherm, and below T_c by the difference Δρ = (ρ_BW − ρ)_water to the triple point.

All other high-density liquid-side thermodynamic properties could be obtained from the rigidity isotherms, via the equalities in Equation (2) for all temperatures, including Gibbs energies and two-phase regions and coexistence lines. Other thermodynamic state functions, e.g. Gibbs energies that determine phase coexistence boundaries thermodynamic properties can likewise be prescribed in terms of the various physical constants for water at temperatures up to T_B and 1000 MPa. In the following sections of this report, however, we will focus on the rigidity symmetry of argon, as the exemplary simple liquid, and its relationship to the percolation lines PA and PB, and the Boyle line.

All phase transition lines, and 2-phase coexistence regions, on a Gibbs p-T surface, for example, are determined by the Gibbs energy state function; two distinct states of different density (or molar volume) have the same T, p and molar Gibbs energy (chemical potential). Van der Waals critical point hypothesis can be tested simply by comparing theory, i.e., van der Waals Equation Gibbs energy, with experimental, i.e. Gibbs energy along the critical isotherm (151 K) for argon from NIST thermophysical property web book that uses TSW Equation-of-state [6] [14] (Figure 4). The van der Waals Gibbs energy from Equations (1) and (2)

G * = R T [ b b − V − ln ( 1 − b V ) − 2 a V ] (3)

in which G * is the excess Gibbs energy relative to the ideal gas at the same T, p.

ΔG/RT for the critical isotherm of argon, referenced to the critical line constant value G_c, is shown in Figure 6, between the maximum coexisting gas density and minimum coexisting liquid densities at T_c for the NIST [6] critical isotherm (151 K). This accurate experimental description of the critical isotherm can be compared with van der Waals singularity prediction in the most favourable comparison, i.e. when the two constants a and b are exactly fitted to correctly predict the critical state point T_c − P_c. Then we obtain the van der Waals V_c for argon that corresponds to a singular critical density ρ_c of 11.0 mol/l, i.e. slightly below the maximum coexisting gas density

The van der Waals hypothesis completely misses the essential physics of critical point (T − p) thermodynamics [7] [8] . The hard-sphere reference model implicitly determines the structure in mean-field and perturbation theories. Since the original van der Waals’ hypothesis, countless generic variations have also failed. All such theories of simple liquids neglect an essential symmetry between gas and liquid states, arising from the cluster physics description, especially in the vicinity of the critical point T_c, p_c.

Near-critical coexistence properties involve hetero-phase fluctuations and the supercritical mesophase, determined by clustering effects and manifested as percolation transitions with discontinuities in density fluctuations or rigidity as given by Equation (2). Mean-field and first-order perturbation theories are only quantitatively successful nearer to the triple point where hetero-phase fluctuations are minimal. Sedunov [15] has investigated the importance of molecular clustering equilibria in atomic (argon), and molecular (CO₂ and H₂O) gases, and reported that these effects play an important part of the description of thermodynamic properties of all real gases, and hence also gas-liquid phase transitions. Gibbs energy differences are the driving force for all first-order phase transitions. Figure 6 shows that van der Waals Equation (1) gets the science of critical coexistence completely wrong.

A more significant observation from the experimental Gibbs energy critical isotherm in Figure 6, is that the symmetry between states below the maximum coexisting gas density, and states above the minimum coexisting liquid density applies to Gibbs energies. Between these two physical constant state points, determined by the intersection of percolation lines, T_c, p_c, and G_c (Gibbs chemical potential) are all constant. At the critical line, the rigidity is zero as the density fluctuations in Equation (2) diverge. We can see from Equation (2) that this symmetry in G(p,T) relates to the state function rigidity (ω) and to the same density fluctuations in both gas and liquid phases at T_c.

Rigidity symmetry has its origins in the statistical cluster physics of real gases that is mirrored by the cluster physics of voids or vacancies, i.e. available volume, in liquids. The van der Waals mean-field approximation in Equation (1) and all similar mean-field theories of liquids, and perturbation theories of hard sphere fluid reference state [16] all neglect this essential physics that determines the thermodynamic state functions and Equation-of-state of both gases and liquids [9] . Real gases are composed of clusters of atoms or molecules, even at very low finite densities, to some extent, for all temperatures below T_B.

Any real gas below T_B is a multicomponent mixture of monomers, dimers, trimers etc. [15] . Each species obeys the ideal gas law of partial pressures at a sufficient low density. The equilibrium constants k_n for multiple molecular clusters, e.g., (H₂O)_n or (CO₂)_n or atomic clusters, e.g., argon (Ar)_n, denoted generally by A_n, can be expressed as sequence of gas phase chemical reactions according to the equilibria: nA ⇔ A_n. The equilibrium constants can be expressed as a series in which [A₁] is the monomer density fraction and [A_n] fraction of cluster size n.

Then

k 2 = [ A 2 ] / [ A 1 ] 2 ; k 3 = [ A 3 ] / [ A 1 ] 3 ; k n = [ A n ] / [ A 1 ] n (4)

At low density, the partial pressures of [A_n] from Dalton’s law can be summed as a series for the cluster density species (ρ_p) at total pressure (p), then

p = ρ p R T = [ A 1 ] + k 2 [ A 1 ] 2 + ⋯ + k n [ A 1 ] n + ⋯ (5)

ρ R T = [ A 1 ] + 2 k 2 [ A 1 ] 2 + ⋯ + n k n [ A 1 ] n + ⋯ (6)

substituting from Equation (6) in Mayer expansion for pressure in terms of the atom density powers, ρ⁽ⁿ⁻¹⁾ that define the virial coefficients b_n [16]

p = ρ R T ( 1 + b 2 ρ + b 3 ρ 2 + ⋯ + b n ρ n + ⋯ ) (7)

by combining terms, we obtain the relationships between coefficients b_n and K_n

b 2 = − k 2 (8)

b 3 = 4 k 2 2 − k 3 (9)

b 4 = 18 k 2 k 3 − 20 k 2 3 − 3 k 4 (10)

These relationships hold for all the b_n(T) and k_n(T) for all T < T_B. Since all the k_n(T) are everywhere positive, there must be a significant cancellation, to some unknown extent, of the higher virial terms in the Mayer cluster expansion Equation (7). Only b₂(T) and b₃(T), of argon for example, are required to represent accurate gas pressures in the range from T_B > T > 0 at densities below the percolation line ρ_PB and for all isotherms below T_c for all densities below the gas-liquid and gas-solid coexistence lines down to zero K. The cancellation of b₄ is already evident for all T > T_c (151 K) as seen in Figure 7.

Accurate experimental values of b₂(T) and b₃(T) (Figure 7) have recently been reported for argon from sound velocity (c) measurements in the temperature range 100 to 500 K [17] . Using known b₂ and b₃ values, we can obtain b₄(T) in the same T-range given also the NIST experimental heat capacity and sound velocity data for argon. By plotting [ω/(RT) − (1 + 2b₂ρ + 3b₃ρ²)] versus ρ³ we obtain the b₄(T) values also shown in Figure 7.

The Mayer virial series [16] , Equation (7), is a Taylor expansion for pressure derivatives in powers about zero density, whence ‘bond’ lengths within clusters that determine k_n become negligible compared to divergent correlation lengths between clusters that determine the density in Equation (5). Hence, the concept of rigidity symmetry [18] means that the liquid properties can all be determined from the corresponding-state gas phase given only the lower virial coefficients. We can now proceed to specify the thermodynamic state functions, notably, the Boyle and critical and triple point temperatures, BW and/or RS lines, and the coexisting percolation densities at T_c.

We note that b₃(T) and b₂(T) appear to be linearly related for T > T_c. and contain information on T_c. b₃(T) shows a maximum at T_c whereas b₄ goes to zero for all T > T_c. All the higher virial coefficients n > 4 either cancel similarly or will become negligible at the low densities below the ρ_PB line. Hence, we can determine physical constants and thermodynamic Equations-of-state from only the lower virial coefficients b₂ and b₃ for the gas phase.

Both the BW and RS lines extend to hypothetical amorphous and crystalline solid states, i.e. insofar as they would obey classical statistical mechanics at the lower temperatures. The neglect to a large extent of the higher terms b_n ≥ b₄ in the virial expansion can be justified by an analysis of the expansion of the gas pressure in terms of equilibrium constants defined in the low-density limit obedience to Dalton’s law of partial pressures for argon. We do not yet know whether this is also the case for more complex molecular liquids CO₂ or water, probably not.

The percolation pressures, of bound clusters in the gas, and of gaseous voids in the liquid, with decreasing T, intersect to trigger a critical point coexistence line at T_c and a supercritical mesophase with linear hybrid properties (Figure 3(b)). The percolation transitions are higher-order phase transitions that delineate the gas phase below the Boyle temperature when the clusters of “liquid-in-gas” diverge to percolate the phase volume. There are no phase transitions for all gas densities below the PB-line density of gaseous bonded clusters ρ_PB. The gas phase Equation-of-state is given by the Mayer virial expansion, for given T and for ρ < ρ_PB we have the following, formally exact up to the first thermodynamic discontinuity, Mayer cluster expansions [16]

Work

w = ( p ρ ) T = R T ( 1 + b 2 ρ + b 3 ρ 2 + ⋯ + b n ρ n − 1 ) (11)

Rigidity

ω = ( d p d ρ ) T = R T ( 1 + 2 b 2 ρ + 3 b 3 ρ 2 + ⋯ + n b n ρ n − 1 ) (12)

Solidity

σ = ( d 2 p d ρ 2 ) T = R T ( 2 b 2 + 6 b 3 ρ + ⋯ + n ( n − 1 ) b n ρ n − 2 ) (13)

The Boyle work ratio for the critical isotherm (151 K) of argon is plotted in Figure 8. Both work (w) and rigidity (ω) decrease with increasing density for a gas and mesophase densities below PA; both increase with density for the liquid phase above a minimum very slightly greater than ρ_PA(T_c). The rigidity, ω = RT, however, is more convenient reference point in describing Equations-of-state and Gibbs energies for phase transitions. Its derivative, solidity σ, Equation (13) is −ve for a gas, zero in the mesophase, and +ve for liquid phase. We can use these Equations to show that there must exist a maximum coexisting gas-phase density along the percolation line PB, at state point whereupon both ω and σ go to zero at T_c [7] [8] .

All points on the gas-phase percolation line PB, including the maximum coexisting gas density at T_c, occur when the solidity (σ) is set to zero in Equation (13) and all terms n > 3 neglected, then we have

3 ρ P B ( T c ) = − ( b 2 / b 3 ) T c (14)

i.e. a very simple Equation for the maximum coexisting gas density at T_c that can be shown to be very close to experimental reality. The ratio −(b₂/b₃)_T (Figure 9) is plotted from the data of Estrada-Alexanders et al. (shown in Figure 4 above) and seen to be linear in a 200 K temperature range beyond which it passes through zero at T_B and goes negative. Over this temperature range, it can be represented by a single ground-state density constant that determines −(b₂/b₃)_T in using the T → 0 ground-state constant from the linear region that T → T B as illustrated in Figure 9. If the value at T_c is used, a slightly higher ground-state density is obtained.

Thus, if the terms b_n > 3 in Equations (13) and (14) are negligible for the gas phase below the PB line, the result can be used to confirm the experimental observation that the ω goes to a constant and that the solidity goes to zero at −(b₂/3b₃)_T. The ratio is obtained from Figure 9 at the zero-density intercept −(b₂/b₃)₀ = −0.1162T + 47.34 mol/l with regression (R²) for the range 300 - 403 K = 0.9979. This result corresponds to a maximum coexisting gas density at T_c of 10.1. This is slightly lower, but of the same order as the maximum reported experimental coexisting gas density 11.4 mol/l by Michels et al. [19] or 11.8 mol/l by Gilgen et al. [20] .

Likewise, Equation (11) for the BW line can be used to obtain the minimum coexisting liquid density, again, from Figure 8, Boyle work w(ρ)_T goes to a minimum at the density ρ_PA(T_c). Then, b₂ + 2b₃ρ_PA = 0 at T_c, resulting in the simple equality again that the minimum coexisting liquid density at T_c is given

by ρ P A ( T c ) = − 1 2 ( b 2 / b 3 ) T c . Using the ground-state constant 47.34 mol/l to define

the T_B asymptotic slope of −(b₂/b₃)_T data in Figure 9, we obtain a value ρ_PA(T_c) = 14.7 mol/l. This result is reassuringly close to the value obtained from NIST [6]

(Figure 4) ~14.9 mol/l and near to the minimum recorded coexisting liquid densities of Michels et al. (15.35 mol/l) [19] and Gilgen et al. (15.07 mol/l) [20] .

The condition p/ρ_B = RT defines the BW line that connects all these state points of both the super- and sub-critical liquid along any isotherm below T_B. If we denote the density of the Boyle-work line ρ_BW(T), the linearity can be explained by considering the form of a rigidity symmetry line, which we will denote by ρ_RS(T). Now, we have a relationship between these two lines that turns out to be quite simple for argon.

The RS line, defined by the equality [18]

(dp/dρ)_T = RT (15)

has its origins in the symmetry of gas and liquid density fluctuations which are equivalent to ideal gas density variance along this line (Equation (2). Again, from the rigidity virial expansion Equation (6) we see a simple prediction. If the isotherm were to be perfectly symmetric, then the virial expansion that defines the rigidity for the gas below PB-line can be applied for liquid-state densities between the PA-percolation line and the rigidity symmetry line ρ_RS(T). Then, the rigidity for

ρ P A < ρ < ρ R S

ω = R T ( 1 + 2 b 2 Δ ρ + 3 b 3 Δ ρ 2 + ⋯ + n b n Δ ρ n − 1 ) (16)

where Δρ = (ρ_RS −ρ)_T. The RS line ρ_RS(T), when Δρ = zero, decreases linearly with T. Along any isotherm the symmetry can be shown to extend to the BW line density ρ_BW(T). Since for all densities beyond ρ_PA(T) there are no phase transitions of any order, both the Boyle work ratio w(T) and rigidity ω(T) are continuous in all their density derivatives along the respective lines to the first-order phase transitions on condensation. If all the higher terms n ≥ 4 in the Equations (11)-(13) are negligible by cancellation for densities below ρ_PB, then, for the BW line

w = R T ( 1 + b 2 Δ ρ + b 3 Δ ρ 2 ) (17)

when Δρ = (ρ_BW − ρ)_T. Then from (16) and (17), neglecting all b_n terms n > 3,

ρ R S ( T ) = 2 ρ B W ( T ) / 3 (18)

It follows from Equation (18) that the BW line (p/ρ_B = RT) will relate to the RS line, dp/dρ_RS = RT, for all supercritical liquid-side states essentially exactly for lower densities above T_c. In the following sections, we establish empirically that the relationship is accurate over the whole T-range for argon from T_B to the hypothetical ground-states of BW and RS lines at T → 0 .

A selection of ω(T) isotherms for argon from NIST web book [6] is shown in Figure 10 for the temperature range T_c to T_B. The densities corresponding to ω(T) and w(T) can be obtained very accurately at the points ρ_RS(T) and ρ_BW(T)

and are seen to be linear. The Boyle line is perfectly linear over the entire range with a slope that is consistent with the result in Equation (14). The BW ρ_BW(T) is essentially the same as −b₂/b₃(T) in Figure 9, with the same constant ground-state of 47.0 ± 0.5 mol/l. This is a remarkable equality: ρ_BW(T) = −(b₂/b₃)_T relating the BW line to only the lower virial coefficients for T_c < T < T_B.

The BW line ρ_B(T) is empirically found to be near perfectly linear for argon from NIST data [6] . When an EXCEL trendline is fitted to the intersections whence p/ρ_B = RT below T_B, as shown in Figure 10, we obtain the linear trendline

T = 8.5881 ρ + 403.26 K ( regression 〈 R 2 〉 = 0.9996 )

to estimate the Boyle temperature (403.3 ± 0.5 K) and ground-state “crystal” constant (46.96 ± 0.05 mol/l).

The Boyle line describes a line of states for which all the virial coefficients in Equation (4) cancel. Since a straight line is continuous with all its higher derivatives zero, it is not surprising that although the BW line describes unstable states (within 2-phase regions) below about 91 K when it hits the liquid-to-FCC freezing transition, it terminates at a perfect classical close-packed crystal ground state characteristic density determined by the pair-potential Hamiltonian.

The intercept of the rigidity symmetry line at T = 0 (32.5 mol/l) is closer to a frozen liquid state of amorphous packing of argon atoms in the liquid density range. Random close packed (RCP) density 2/π (0.6366) would correspond to a hard-sphere bond diameter of the argon dimer 0.3915 nm. The ρ_RS ground-state density constant for argon, however, is closer to triple-point liquid random loose packing, with a packing fraction around 50%, calculated from the experimental Ar₂ dimer bond length, and 1/3 of maximum crystal packing (74%).

An analytical theory of simple liquids, without adjustable parameters, seems now within reach: i.e. to relate the Ar₂ pair-potential Hamilton to the p(ρ,T) Equations-of-state in the regions of the phase diagram delineated by the lines PB, PA, RS and BW all of which are now defined by b₂(T) and the linear ratio −b₂/b₃(T), obtainable from BW-line, of the phase diagram, over the whole density-temperature range.

The fundamental objective of the theory of simple liquids [16] is to relate the intermolecular or interatomic forces that define the Hamiltonian of the system, to the p(ρ,T) Equation-of-state. The pair potential for argon has been extensively studied, probably more so than any other exemplary fluid, and is known quite accurately both from original experiment [19] [20] [21] and more recently, ab initio quantum theory [22] . It is characterized, often only by 2 parameters e.g., Lennard-Jones, i.e. by the range of the minimum energy at the distance r₀ of zero force. The experimental value is r₀(Ar₂) = 0.3704 ± 0.005 nm, based upon the more accurate functional representative of Boyes [21] .

Assuming that the argon BW-line ground state is a perfect FCC or HCP close-packed lattice of spheres in the BW-crystal structure, we can calculate the ρ B W ( T → 0 ) constant from the reduced maximum packing density of spheres ρ * = N r 0 3 / V = 2 1 / 2 . Substituting the argon dimer bond length, we obtain a prediction of the ρ B W ( T → 0 ) = 46.21 mol/l.

It appears that the cluster analysis in section 2 above contains information on the maximum packing of argon atoms. This is understandable from the cluster physics analysis in section 2. If all the equilibrium constants k_n were to be known, they would reveal this limiting, hypothetical, close-packed crystal density constant. The virial expansion, evidently, has its first pole at the maximum packing density of minimum energy.

This density obtained from the pair potential agrees well with the constant obtained from Figure 9, −(b₂/b₃)_T ratio, and with the interpolation in Figure 10 of the BW line to T → 0 (ρ_B0 = 46.96 mol/l). It is still, however, somewhat greater than the experimental HCP-argon crystal value 44.43 mol/l [23] . A small difference between the Boyle line hypothetical ground state physical constant could arise zero-point energy quantum effects in real crystal states. Argon undergoes an equilibrium FCC to HCP phase transition at a temperature around 35 K along its equilibrium experimental (p/ρ_B)_T BW line [23] .

Using the experimental co-existence envelope data from NIST, for the present, we can construct an accurate phase diagram that enables the bounds of the p(ρ,T) Equations-of-state to be quantified. There are no arbitrary parameters other than the virial coefficients b₂(T) and b₃(T) and the physical constants that they determine. The Boyle temperature T_B is determined by b₂(T): when it changes sign from −ve to +ve. The BW line ground state density is then equivalent to the (−b₂/b₃)_T line, linear from T = T_B. The value obtained in Figure 5 for the scaling ground-state constant is 47.34 mol/l. This compares favorably with the Kihara pair-potential value for the minimum energy of the FCC or HCP crystal 46.21 mol/l. The experimental constant obtained from BW-line isotherms is 46.96 mol/l (Figure 10).

This ground-state constant, determined also from the virial coefficients, can be used to sketch an accurate phase diagram (Figure 11) using the various simple equalities derived above. The ratio −(b₂/b₃)_T, below T_B, determines the BW line ground-state constant for argon. Given the simple relationships between PA, PB, RS, and BW(T), we can determine the critical temperature T_c (whence ω(T) → zero at ρ_PA(T) or ρ_PB(T), and then fill in the isotherms of p(T), w(T), or ω(T) over the temperature range from the triple point to the BW line and beyond, to the state points above the BW line below T_B.

The second observation from the argon phase diagram is that the equilibrium regions of the BW and RS lines completely exist only within a single Gibbs supercritical “liquid” phase with P = 1. Whereas the percolation transitions delineate the supercritical gas and liquid regions by higher-order phase transitions, the BW and RS lines have no phase transitions and are therefore continuous in all their derivatives. Thus, both lines are defined by their ground state physical constant hypothetical densities obtained in linear interpolation limit that T → 0 .