A method for quantitatively calculating the transformation process of albite particles based on the silica release model

Abstract

The present invention relates to the field of petroleum exploration technology, and more specifically, to a method for quantitatively calculating the transformation process of albite particles based on a silica release model. This method utilizes thermodynamics to determine the pore fluid properties of various types of water-rock equilibrium during the albite transformation process, and to determine the priority of various water-rock reactions at equilibrium, thereby quantitatively calculating the transformation process of albite particles under different environments and the content of different transformation products during the transformation process. This method has important practical implications for groundwater pollution prevention and control, prediction of favorable deep reservoirs in oil and gas basins, and design of transformation processes for low-permeability oil and gas reservoirs.

Description

Technical Field

[0001] The present invention relates to the technical field of petroleum exploration, and in particular to a method for quantitatively calculating a transformation process of albite particles based on a silica release model. Background Art

[0002] Feldspar is one of the most important rock-forming minerals in the Earth's crust and a crucial component of the sandstone framework in sedimentary basins. The transformation of feldspar particles under acidic fluid environments raises a range of issues, including formation water contamination and prevention, the transformation of deep sandstone reservoirs in petroliferous basins, greenhouse gas (CO2) reinjection, and reservoir alteration during oil and gas development. For nearly a century, geologists have conducted extensive observations and tests on surface weathering residues of feldspar minerals in various rocks, the transformation of feldspar in laboratory acidic solutions, and sandstone reservoir samples from petroliferous basins. Scholars have widely used this model to explain the composition of feldspar weathering residues under surface weathering conditions. However, controversy remains regarding whether this model can explain the transformation of feldspar particles under low-pH fluid environments and high-temperature environments. Furthermore, quantitative calculations of feldspar transformation processes under acidic fluid environments are relatively scarce, hindering the prediction of deep sandstone reservoirs in petroliferous basins.

[0003] Currently, there are no studies or reports on the quantitative calculation of the transformation process of albite particles under different environments and the content of different transformation products during the transformation process based on the silica release model. Summary of the Invention

[0004] The main purpose of the present invention is to provide a method for quantitatively calculating the transformation process of sodium feldspar particles based on a silica release model. The present invention uses thermodynamics to determine the properties of pore fluids when various types of water-rock reach equilibrium during the transformation process of sodium feldspar, and to determine the priority of various water-rock reactions when they reach equilibrium, thereby achieving quantitative calculation of the transformation process of sodium feldspar particles under different environments and the content of different transformation products during the transformation process.

[0005] To achieve the above object, the present invention adopts the following technical solutions:

[0006] The present invention provides a method for quantitatively calculating the transformation process of albite particles based on a silica release model, which comprises the following steps:

[0007] Identify all water-rock reaction types during the transformation of albite grains in an acidic fluid environment under the silica release model;

[0008] Calculate the molar Gibbs energy of formation of solid phase and solvent using the constant pressure specific heat model;

[0009] The HKF model is used to calculate the molar Gibbs energy of formation of water-soluble particles formed during the transformation of albite. The Gibbs equation is used to determine the equilibrium constants of different reactions. The equilibrium constants are used to determine the concentrations of various particles in aqueous solutions at the equilibrium stage of various water-rock reactions under different pH values, temperatures, and pressures.

[0010] According to the conditions of aqueous solution at different water-rock reaction equilibrium periods, the order in which different water-rock reactions reach equilibrium is determined;

[0011] Based on the order in which water-rock reactions reach equilibrium, the transformation path of albite under different temperature and pH environments and the content of transformation substances of different genesis under different environments are determined.

[0012] Furthermore, under the silica release model, the water-rock reactions during the transformation of albite particles in an acidic fluid environment include:

[0013] Reaction 1: NaAlSi3O8(s)+(0-1)H + (aq)+H2O(l)→H (0-1) Na (1-0) AlSi3O8(s)+(1-0)Na + (aq);

[0014] Reaction 2: 3NaAlSi3O8(s)+2H + (aq)+12H2O(l)→Na[AlSi3O 10 ]Al2(OH)2(s)+6H4SiO4(aq)+2Na + (aq);

[0015] Reaction 3: 2Na[AlSi3O 10 ]Al2(OH)2(s)+2H+(aq)+3H2O(l)→2Na+(aq)+3Al2[Si2O5](OH)4(s)(kaolinite);

[0016] Reaction 4: Al2[Si2O5](OH)4(s)+5H2O(l)→2Al(OH)3(s)(hydrous aluminum oxide residue)+2H4SiO4(aq);

[0017] Reaction 5: Al(OH)3(s)→Al(OH)3(aq);

[0018] Reaction 6: Al(OH)3(aq)+H+(aq)→Al(OH)2+(aq)+H2O(l);

[0019] Reaction 7: Al(OH)3(aq)+2H+(aq)→Al(OH)2+(aq)+2H2O(l);

[0020] Reaction 8: Al(OH)3(aq)+3H+(aq)→Al 3+ (aq)+3H2O(l);

[0021] Reaction 9: Al(OH)3(aq)+H2O(l)→Al(OH)4 - (aq)+H + (aq);

[0022] Reaction 10: H4SiO4(aq)→H3SiO4 - (aq)+H + (aq);

[0023] Reaction 11: H3SiO4 - (aq)→H2SiO4 2- (aq)+H + (aq);

[0024] Reaction 12: Na + (aq)+H3SiO4 - (aq)→NaH3SiO4(aq);

[0025] Reaction 13: 2Al(OH)3(aq)+2H4SiO4(aq)→Al2[Si2O5](OH)4(s)(kaolinite)+5H2O(l);

[0026] Reaction 14: H4SiO4(aq)→SiO2(s)+2H2O(l);

[0027] Reaction 15: Na + (aq)+3Al(OH)3(aq)+3H4SiO4(aq)→Na[AlSi3O 10 ]Al2(OH)2(s)+H+(aq)+9H2O(l).

[0028] Furthermore, the order in which different water-rock reactions reach equilibrium is:

[0029] When the temperature is below 373.15K, reaction 4 reaches equilibrium first. At 373.15-393.15K and pH = 1-5, reaction 4 reaches equilibrium first. At 373.15-388.15K and pH = 6, reaction 4 reaches equilibrium first. At 388.15-393.15K and pH = 6, reaction 3 reaches equilibrium first. At 373.15-393.15K and pH = 7, reaction 3 reaches equilibrium first. When the temperature is above 393.15K, reaction 3 reaches equilibrium first.

[0030] Furthermore, when the temperature is lower than 393.15K, no quartz precipitation occurs when Reaction 4 reaches equilibrium. Regarding the priority between Reaction 4 equilibrium and the development of hydrous aluminum oxide residues, as the pH of the solution increases, the temperature range in which hydrous aluminum oxide residues exist when Reaction 4 reaches equilibrium gradually increases:

[0031] When pH = 1-2, no hydrated aluminum oxide residues are left when reaction 4 reaches equilibrium within this temperature range; when pH = 3, the appearance of 363.15K-393.15K hydrated aluminum oxide residues is earlier than the equilibrium of reaction 4; when pH = 4, the appearance of 323.15K-393.15K hydrated aluminum oxide residues is earlier than the equilibrium of reaction 4; when pH = 5, the appearance of 300.15K-393.15K hydrated aluminum oxide residues is earlier than the equilibrium of reaction 4; when pH = 6-7, the appearance of 273.15K-393.15K hydrated aluminum oxide residues is earlier than the equilibrium of reaction 4.

[0032] Furthermore, in the temperature range of 273.15K-393.15K and pH=1-7, no kaolinite precipitation occurs during the equilibrium period of reaction 4, nor does the hydrous aluminum oxide residue appear.

[0033] Furthermore, when the temperature is higher than 393.15K, reaction 3 reaches equilibrium first. In the low temperature and low pH fluid environment, the reaction is more likely to develop authigenic quartz precipitation before reaction 3 reaches equilibrium. As the pH value of the solution increases, the temperature range for the preferential appearance of quartz precipitation decreases: when pH = 1, 393.15K-548.15K; when pH = 2, 393.15K-513.15K; when pH = 3, 393.15K-468.15K; when pH = 4, 393.15K-438.15; when pH = 5, 393.15K-413.15K. Quartz precipitation already exists when reaction 3 reaches equilibrium.

[0034] In other pH and temperature ranges, no quartz minerals precipitate before reaction 3 equilibrium;

[0035] When pH=1, 513.15K-593.15K; when pH=2, 423.15K-593.15K; when pH=3,

[0036] 543.15K-623.15K; when pH = 4, 393.15-543.15K; when pH = 5, 393.15-483.15K; when pH = 6, 393.15-443.15K; when pH = 7, 373.15-403.15K; it is manifested that boehmite precipitation occurs preferentially before reaction 3 reaches equilibrium.

[0037] Furthermore, there is no kaolinite precipitation before the reaction 3 equilibrium, quartz precipitation and hydrous aluminum oxide residue.

[0038] Furthermore, under the silica release model, the transformation pathways of albite particles in an acidic fluid environment include:

[0039] Path A: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → reaction 2 and reaction 3 proceed simultaneously → reaction 2 and reaction 3 proceed simultaneously, quartz precipitates → reaction stops;

[0040] Path B: Reaction 2, Reaction 3, Reaction 4, and Reaction 5 proceed simultaneously → Reaction 2 and Reaction 3 proceed simultaneously → Reaction 2 and Reaction 3 proceed simultaneously, quartz precipitates → Reaction 2 proceeds, quartz precipitates → reaction stops;

[0041] Path C: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously, quartz precipitation → Reaction 2, reaction 3, and reaction 4 proceed, quartz precipitation → Reaction 2, quartz precipitation → reaction stops;

[0042] Path D: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously, quartz precipitation → Reaction 2, quartz precipitation → reaction stops;

[0043] Path E: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → reaction 2, reaction 3, and reaction 4 proceed simultaneously → reaction 2 proceeds → reaction 2, quartz precipitation → reaction stops;

[0044] Path F: Reaction 2, Reaction 3, Reaction 4, and Reaction 5 proceed simultaneously → Reaction 2 proceeds → Reaction 2,

[0045] Quartz precipitation → reaction stops;

[0046] Path G: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously, quartz precipitates → Reaction 2 proceeds, quartz precipitates → reaction stops;

[0047] Path H: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2 proceeds → Reaction 2 proceeds, quartz precipitates → reaction stops;

[0048] Path I: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously → Reaction 2 proceeds → Reaction 2 proceeds, quartz precipitates → Reaction stops;

[0049] Path J: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed → Reaction 2, reaction 3, and reaction 4 proceed together → Reaction 2 and reaction 3 proceed together → Reaction 2 and reaction 3 proceed together, quartz precipitates → Reaction 2 proceeds, quartz precipitates → reaction stops;

[0050] Path K: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously, quartz precipitates → reaction stops;

[0051] Path L: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously, and quartz precipitates → Reaction 2 proceeds, and quartz precipitates → the reaction stops.

[0052] Compared with the prior art, the present invention has the following advantages:

[0053] This method utilizes thermodynamic methods and a silica release model to calculate the transformation process of albite particles and the amounts of different transformation products during albite transformation in an acidic environment. The method is simple and highly applicable, and has important practical implications for groundwater pollution prevention and control, prediction of favorable deep reservoirs in oil and gas basins, and design of transformation processes for low-permeability oil and gas reservoirs. BRIEF DESCRIPTION OF THE DRAWINGS

[0054] The accompanying drawings, which constitute a part of the present invention, are used to provide a further understanding of the present invention. The exemplary embodiments of the present invention and their descriptions are used to explain the present invention and do not constitute improper limitations on the present invention.

[0055] Figure 1 Equilibrium constants for some water-rock reactions in the silica release model;

[0056] Figure 2 In actual cases, the Na required for the equilibrium of reaction 2 is + (aq) concentration;

[0057] Figure 3 In actual cases, the Na required for the equilibrium of reaction 3 is + (aq) concentration;

[0058] Figure 4 Na in the equilibrium period of reaction 2 and reaction 3 under the total pressure of 20 MPa + (aq) / H + (aq) molar concentration ratio;

[0059] Figure 5 The equilibrium priority of reaction 3 and reaction 4 under different pH conditions at a total pressure of 20 MPa;

[0060] Figure 6 The priority of reaction 4 equilibrium and quartz precipitation under different pH environments at a total pressure of 20 MPa;

[0061] Figure 7 The priority of reaction 4 equilibrium, quartz precipitation and aluminum-containing hydrated oxide residues under different pH conditions at a total pressure of 20 MPa;

[0062] Figure 8 The priority of reaction 4 equilibrium, quartz precipitation, the appearance of aluminum-containing hydrous oxide residues and kaolinite precipitation under different pH environments at a total pressure of 20 MPa;

[0063] Figure 9 The priority of reaction 3 equilibrium and quartz precipitation under different pH environments at a total pressure of 20 MPa;

[0064] Figure 10 The priority of the reaction 3 equilibrium, quartz precipitation and aluminum-containing hydrated oxide residues under different pH environments at a total pressure of 20 MPa;

[0065] Figure 11 The priority of the occurrence of reaction 3 equilibrium, quartz precipitation, aluminum-containing hydrated oxide residue and kaolinite precipitation under different pH environments at a total pressure of 20 MPa;

[0066] Figure 12 Transformation process of albite particles in acidic fluid environment based on silica release model. DETAILED DESCRIPTION

[0067] It should be noted that the following detailed descriptions are exemplary and intended to provide further explanation of the present invention. Unless otherwise specified, all technical and scientific terms used herein have the same meaning as commonly understood by those skilled in the art to which the present invention belongs.

[0068] It should be noted that the terms used herein are only for the purpose of describing specific embodiments and are not intended to limit exemplary embodiments according to the present invention. As used herein, unless the context clearly indicates otherwise, the singular form is also intended to include the plural form. In addition, it should be understood that when the terms "comprising" and / or "including" are used in this specification, they indicate the presence of features, steps, operations and / or combinations thereof. In order to enable those skilled in the art to more clearly understand the technical solution of the present invention, the technical solution of the present invention will be described in detail below in conjunction with specific embodiments.

[0069] Example 1

[0070] The method for quantitatively calculating the transformation process of albite particles based on a silica release model comprises the following steps:

[0071] Step 1: Determine all water-rock reaction types during the transformation of albite particles in an acidic fluid environment under the silica release model, as shown in Table 1:

[0072] Table 1

[0073]

[0074]

[0075] Step 2: Calculate the molar Gibbs energy of formation of the solid phase and the solvent using the constant pressure specific heat model (Formula 1).

[0076]

[0077] Among them: G P,T is the Gibbs energy of molar formation of various substances under the conditions of P (pressure) and T (temperature); H P,T is the molar formation enthalpy of the substance under the conditions of P (pressure) and T (temperature); S P,T is the molar entropy of formation of a substance under the conditions of P (pressure) and T (temperature); r 0.1Mpa; T r is 298.15K; Cp is the constant pressure specific heat capacity of different substances, which can be expressed as Cp = a + b * T + c / T 2 The various parameters of related substances in the calculation process are based on Table 1.

[0078] Step 3: Use the HKF model (Formula 2) to calculate the molar Gibbs energy of formation of the water-soluble phase particles formed during the transformation of albite.

[0079]

[0080] Where j represents the jth solute component in the aqueous solution. P and T are the pressure (bar) and temperature (K) of interest; Pr and Tr are the reference pressure (1 bar) and reference temperature (298.15K). r =2600(bar);T r = 228 (K). a1-a4, c1-c2 are the fitting parameters of the characteristic ions in the solution. ε is the dielectric constant of pure water. Y is the derivative of the dielectric constant of pure water with respect to temperature (K). is the Born coefficient of particles in aqueous solution, which is itself a function of ionic charge, effective radius, temperature, pressure and the pure water property g.

[0081] Step 4: Use the Gibbs equation (Formula 3) to determine the equilibrium constants of different reactions ( Figure 1 ).

[0082]

[0083] in represents the Gibbs energy change under the environment of T (K) and P (Mpa); R is the molar gas constant, R = 8.314 J / (mol*K); K is the equilibrium constant during the reaction equilibrium period.

[0084] Step 5: Use the equilibrium constant to determine the concentration of various particles in the aqueous solution at the equilibrium period of various water-rock reactions under different pH values, different temperatures, and different pressures.

[0085] Step 6: Based on the aqueous solution conditions at different water-rock reaction equilibrium periods, determine the order in which different water-rock reactions reach equilibrium.

[0086] Assume that a precipitation reaction reaches equilibrium first, i.e., a certain reactant appears. Based on the concentrations of other particles under these conditions calculated in Step 5, we can then compare the priority of this reaction with the other reactions at the time of equilibrium, i.e., the priority of each new mineral precipitation. By comparing each reaction one by one, we can determine the priority of the appearance of different precipitates.

[0087] According to the silica release model of albite, the silica contained in albite particles is released in stages, forming sodium mica (reaction 2), kaolinite (reaction 3) and hydrous aluminum oxide residue (reaction 4). The silica released by the reaction enters the aqueous solution and undergoes a series of hydration, ionization and ion combination reactions to form H4SiO4(aq), H3SiO4 - (aq), H2SiO4 2- (aq) and NaH3SiO4(aq) (reactions 10 / 11 / 12), after reaching a certain concentration, precipitation occurs in the form of quartz crystals, kaolinite or sodium mica (reactions 13 / 14 / 15). The hydrous aluminum oxide residue (gibbsite) formed during the reaction will also dissolve and form Al(OH)4 - (aq), Al(OH)3(aq), Al(OH)2 + (aq), Al(OH)2 + (aq) and Al3 + (aq) in the aqueous solution (reactions 6 / 7 / 8 / 9) until saturation is reached, at which point the hydrous aluminum oxide residue will no longer dissolve (reaction 5). At the same time, Al(OH)3(aq) in the aqueous solution may also react with H4SiO4(aq) or Na + (aq) combines and precipitates as kaolinite or paragonite (reaction 13).

[0088] Based on the silica release model of albite, the order in which various reactions occur and stop determines the transformation process of albite. Therefore, we first explore the priority of achieving equilibrium between reactions 2, 3, and 4 under different temperature and pH environments, and then explore the priority of the occurrence of various mineral precipitations and the equilibrium between reactions 2, 3, and 4.

[0089] Regarding the priority of reaction 2 and reaction 3, the study shows that the equilibrium priority of reaction 2 and reaction 3 is only controlled by temperature, and the H+(aq) concentration has almost no effect on it; when the temperature is lower than 298.15K, the Na+(aq) concentration required for the equilibrium of reaction 3 is higher than the Na+(aq) concentration required for the equilibrium of reaction 2, and reaction 2 reaches equilibrium earlier than reaction 3; when the temperature is higher than 298.15K, the Na+(aq) concentration required for the equilibrium of reaction 3 is lower than the Na+(aq) concentration required for the equilibrium of reaction 2, and reaction 3 reaches equilibrium earlier than reaction 2 ( Figure 2-Figure 4 ).

[0090] Regarding the priority of Reaction 2 and Reaction 4, the study shows that: when the temperature is lower than 398.15K, the H4SiO4(aq) concentration required for the equilibrium of Reaction 4 is lower than the H4SiO4(aq) concentration required for the equilibrium of Reaction 2 and quartz precipitation, that is, Reaction 4 reaches equilibrium earlier than Reaction 2; when the temperature is higher than 398.15K, the H4SiO4(aq) concentration required for the equilibrium of Reaction 4 is higher than the H4SiO4(aq) concentration required for quartz precipitation, that is, Reaction 4 will never reach equilibrium, and the cessation of Reaction 4 is when the product of Reaction 3 (kaolinite) is completely consumed.

[0091] Comparing the priorities of reaction 3 and reaction 4, the study shows that when pH is 1-7 and temperature is ≤373.15K, the H4SiO4(aq) concentration required for equilibrium of reaction 4 is lower than the H4SiO4(aq) concentration in the solution released when equilibrium of reaction 3 and the H4SiO4(aq) concentration required for quartz precipitation, that is, reaction 4 is superior to reaction 3 in stopping ( Figure 5 Figures a to g in the figure); when pH=6 and the temperature is between 373.15-388.15K, the concentration of H4SiO4(aq) required for the equilibrium of reaction 4 is lower than the concentration of H4SiO4(aq) in the solution released when the equilibrium of reaction 3 is reached and the concentration of H4SiO4(aq) required for quartz precipitation, that is, reaction 4 is better than reaction 3 and stops ( Figure 5 f in the figure); pH = 6, temperature between 388.15-393.15K, the H4SiO4(aq) concentration required for the equilibrium of reaction 4 and the quartz precipitation required for the equilibrium of reaction 3 are higher than the H4SiO4(aq) concentration in the solution released when the equilibrium of reaction 3 is reached, that is, reaction 3 is better than reaction 4 and stops ( Figure 5f in the figure); pH = 7, temperature between 373.15-393.15K, the H4SiO4(aq) concentration required for the equilibrium of reaction 4 and the quartz precipitation required for the equilibrium of reaction 3 are higher than the H4SiO4(aq) concentration in the solution released when the equilibrium of reaction 3 is reached, that is, reaction 3 is better than reaction 4 and stops ( Figure 5 g figure in). In summary, when the temperature is lower than 373.15K, reaction 4 preferentially reaches equilibrium; at 373.15-393.15K, pH = 1-5, reaction 4 preferentially reaches equilibrium; at 373.15-388.15K, pH = 6, reaction 4 preferentially reaches equilibrium; at 388.15-393.15K, pH = 6, reaction 3 preferentially reaches equilibrium; at 373.15-393.15K, pH = 7, reaction 3 preferentially reaches equilibrium. When the temperature is higher than 393.15K, reaction 3 preferentially reaches equilibrium ( Figure 5 Figures a to g in the figure).

[0092] When a reaction reaches a preferred equilibrium, the reaction equation can be used to calculate the amount of T(Si) particles released and the amount of residual Al(OH)3(s) formed. Furthermore, based on the equilibrium constants of reactions 5-12, the concentrations of H4SiO4(aq) and Al(OH)3(aq) in aqueous solutions at different temperatures and pH values can be calculated. By comparing these results with the solubility of crystalline quartz, the solubility of hydrous aluminum oxides, and the product of H4SiO4(aq)*Al(OH)3(aq) during kaolinite precipitation, the precipitation priority of residual Al(OH)3(s), quartz, and kaolinite can be determined.

[0093] When the temperature is lower than 393.15K, reaction 4 basically takes precedence in reaching equilibrium, and the equilibrium of reaction 4 takes precedence over the precipitation of other minerals. In this temperature range, the H4SiO4(aq) concentration required for the equilibrium of reaction 4 is lower than the H4SiO4(aq) concentration required for quartz precipitation, that is, when reaction 4 reaches equilibrium, there is no quartz precipitation ( Figure 6 Figures a to g in the figure). The priority of reaction 4 equilibrium and the development of quartz precipitation and hydrous aluminum oxide residue. The study shows that: as the pH of the solution increases, the temperature range in which hydrous aluminum oxide residues exist when reaction 4 is in equilibrium gradually increases; when pH = 1-2, within this temperature range, reaction 4 reaches equilibrium and quartz precipitation occurs without hydrous aluminum oxide residues ( Figure 7 Figure a, Figure b); At pH = 3, the appearance of 363.15K-393.15K hydrous aluminum oxide residues is earlier than the equilibrium of reaction 4 and the precipitation of quartz ( Figure 7 Figure c); At pH = 4, the appearance of the hydrous aluminum oxide residue at 323.15K-393.15K is earlier than the equilibrium of reaction 4 and the precipitation of quartz ( Figure 7d in Figure 5); At pH = 5, the appearance of hydrous aluminum oxide residues at 300.15K-393.15K is earlier than the equilibrium of reaction 4 and the precipitation of quartz ( Figure 7 e in Figure); At pH = 6-7, the appearance of 273.15K-393.15K hydrous aluminum oxide residues is earlier than the equilibrium of reaction 4 and the precipitation of quartz ( Figure 7 f, g). Under the conditions of temperature range and pH=1-7, no kaolinite precipitation occurs when the hydrous aluminum oxide residue appears, the reaction reaches equilibrium, or quartz precipitates, or the hydrous aluminum oxide residue begins to appear. Figure 8 Figures a to g in the figure).

[0094] When the temperature is higher than 393.15K, reaction 3 basically reaches equilibrium first, and the priority of reaction 3 equilibrium over other mineral precipitation. Studies have shown that in low temperature and low pH fluid environment, the reaction is more likely to develop authigenic quartz precipitation before reaction 3 equilibrium; as the pH value of the solution increases, the temperature range for the preferential occurrence of quartz precipitation decreases; when pH = 1, 393.15K-548.15K; when pH = 2, 393.15K-513.15K; when pH = 3, 393.15K-468.15K; when pH = 4, 393.15K-438.15; when pH = 5, 393.15K-413.15K; quartz precipitation already exists when reaction 3 reaches equilibrium ( Figure 9 In other pH and temperature ranges, no quartz minerals precipitate before the equilibrium of reaction 3 ( Figure 9 Figures a to g in the figure). When pH = 1, 513.15K-593.15K; when pH = 2, 423.15K-593.15K; when pH = 3, 543.15K-623.15K; when pH = 4, 393.15-543.15K; when pH = 5, 393.15-483.15K; when pH = 6, 393.15-443.15K; when pH = 7, 373.15-403.15K; it is shown that the hydrous aluminum oxide residue is preferentially present before the reaction 3 reaches equilibrium or the quartz precipitate appears ( Figure 10 There is no kaolinite precipitation before the equilibrium of reaction 3, quartz precipitation and hydrous aluminum oxide residue ( Figure 11 Figures a to g in the figure).

[0095] Step 7: According to the order of water-rock reaction reaching equilibrium, determine the transformation path of albite under different temperature and pH conditions and the content of different genetic transformation substances under different conditions ( Figure 12 ).

[0096] The study shows that there are 12 different transformation pathways of albite under this model ( Figure 12). Mainly includes: Path A: Reaction 2, Reaction 3, Reaction 4, and Reaction 5 proceed together → Reaction 2 and Reaction 3 proceed together → Reaction 2 and Reaction 3 proceed together, and the quartz precipitation reaction stops;

[0097] Path B: Reaction 2, Reaction 3, Reaction 4, and Reaction 5 proceed simultaneously → Reaction 2 and Reaction 3 proceed simultaneously → Reaction 2 and Reaction 3 proceed simultaneously, quartz precipitates → Reaction 2 proceeds, quartz precipitates → reaction stops;

[0098] Path C: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously, quartz precipitation → Reaction 2, reaction 3, and reaction 4 proceed, quartz precipitation → Reaction 2, quartz precipitation → reaction stops;

[0099] Path D: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously, quartz precipitation → Reaction 2, quartz precipitation → reaction stops;

[0100] Path E: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → reaction 2, reaction 3, and reaction 4 proceed simultaneously → reaction 2 proceeds → reaction 2, quartz precipitation → reaction stops;

[0101] Path F: Reaction 2, Reaction 3, Reaction 4, and Reaction 5 proceed simultaneously → Reaction 2 proceeds → Reaction 2,

[0102] Quartz precipitation → reaction stops;

[0103] Path G: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously, quartz precipitates → Reaction 2 proceeds, quartz precipitates → reaction stops;

[0104] Path H: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2 proceeds → Reaction 2 proceeds, quartz precipitates → reaction stops;

[0105] Path I: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously → Reaction 2 proceeds → Reaction 2 proceeds, quartz precipitates → Reaction stops;

[0106] Path J: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed → Reaction 2, reaction 3, and reaction 4 proceed together → Reaction 2 and reaction 3 proceed together → Reaction 2 and reaction 3 proceed together, quartz precipitates → Reaction 2 proceeds, quartz precipitates → reaction stops;

[0107] Path K: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously, quartz precipitates → reaction stops;

[0108] Path L: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously, quartz precipitation → Reaction 2 proceeds, quartz precipitation → reaction stops; different paths appear in different temperature and pH environments, as shown in Table 2.

[0109] Table 2

[0110]

[0111] The above embodiments are preferred implementation modes of the present invention, but the implementation modes of the present invention are not limited to the above embodiments. Any other changes, modifications, substitutions, combinations, and simplifications that do not deviate from the spirit and principles of the present invention should be considered as equivalent replacement methods and are included in the scope of protection of the present invention.

Claims

1. A method for quantitatively calculating the transformation process of albite particles based on a silica release model, characterized in that: The following steps are involved: Identify all water-rock reaction types during the transformation of albite grains in an acidic fluid environment under the silica release model; Calculate the molar Gibbs energy of formation of solid phase and solvent using the constant pressure specific heat model; The molar Gibbs energy of formation of water-soluble particles formed during the transformation of albite is calculated using the HKF model. Use the Gibbs equation to determine the equilibrium constants of different reactions; Using equilibrium constants, we can determine the concentrations of various particles in aqueous solutions at various water-rock reaction equilibrium periods under different pH values, temperatures, and pressures. According to the conditions of aqueous solution at different water-rock reaction equilibrium periods, the order in which different water-rock reactions reach equilibrium is determined; Based on the order in which water-rock reactions reach equilibrium, the transformation path of albite under different temperature and pH environments and the content of transformation substances of different genesis under different environments are determined.

2. The method according to claim 1, characterized in that Under the silica release model, the water-rock reactions during the transformation of albite particles in an acidic fluid environment include: Reaction 1: NaAlSi3O8(s)+(0 - 1)H + (aq)+H2O(l)→H (0-1) Na (1-0) AlSi3O8(s)+(1 - 0)Na + (aq); Reaction 2: 3NaAlSi3O8(s)+2H + (aq)+12H2O(l)→ <h2 style=";text-align:left;direction:ltr">Na[AlSi3O<h2 style=";text-align:left;direction:ltr"> 10 <h2 style=";text-align:left;direction:ltr"> ]Al2(OH)2(s)+6H4SiO4(aq)+2Na<h2 style=";text-align:left;direction:ltr"> + <h2 style=";text-align:left;direction:ltr"> (aq); Reaction 3: 2Na[AlSi3O 10 ]Al2(OH)2(s)+2H+(aq)+3H2O(l)→2Na+(aq)+3Al2[Si2O5](OH)4(s)(kaolinite) Reaction 4: Al2[Si2O5](OH)4(s)+5H2O(l)→2Al(OH)3(s)(hydrous aluminum oxide residue)+2H4SiO4(aq) Reaction 5: Al(OH)3(s) → Al(OH)3(aq) Reaction 6: Al(OH)3(aq)+H+(aq)→Al(OH)2+(aq)+H2O(l) Reaction 7: Al(OH)3(aq)+2H+(aq)→Al(OH)2+(aq)+2H2O(l) Reaction 8: Al(OH)3(aq)+3H+(aq)→Al 3+ (aq)+3H2O(l) Reaction 9: Al(OH)3(aq) + H2O(l) → Al(OH)4 - (aq) + H + (aq) Reaction 10: H4SiO4(aq)→H3SiO4 - (aq)+H + (aq) Reaction 11: H3SiO4 - (aq) → H2SiO4 2- (aq) + H + (aq) Reaction 12: Na + (aq) + H3SiO4 - (aq) → NaH3SiO4(aq) Reaction 13: 2Al(OH)3(aq)+2H4SiO4(aq)→Al2[Si2O5](OH)4(s)(kaolinite)+5H2O(l) Reaction 14: H4SiO4(aq)→SiO2(s)+2H2O(l) Reaction 15: Na + (aq) + 3Al(OH)3(aq) + 3H4SiO4(aq) → Na[AlSi3O 10 Al2(OH)2(s) + H+(aq) + 9H2O(l).

3. The method according to claim 2, characterized in that The order in which different water-rock reactions reach equilibrium: When the temperature is lower than 373.15K, reaction 4 reaches equilibrium first; at 373.15-393.15K, pH=1-5, reaction 4 reaches equilibrium first; at 373.15-388.15K, pH=6, reaction 4 reaches equilibrium first; at 388.15-393.15K, pH=6, reaction 3 reaches equilibrium first; at 373.15-393.15K, pH=7, reaction 3 reaches equilibrium first, and when the temperature is higher than 393.15K, reaction 3 reaches equilibrium first.

4. The method according to claim 3, characterized in that When the temperature is lower than 393.15K, no quartz precipitation occurs when Reaction 4 reaches equilibrium. Regarding the priority between Reaction 4 equilibrium and the development of hydrous aluminum oxide residues: as the pH of the solution increases, the temperature range in which hydrous aluminum oxide residues exist when Reaction 4 reaches equilibrium gradually increases: When pH = 1-2, there is no hydrated aluminum oxide residue when reaction 4 reaches equilibrium within the residual temperature range of hydrated aluminum oxide; when pH = 3, the appearance of 363.15K-393.15K hydrated aluminum oxide residue is earlier than the equilibrium of reaction 4; when pH = 4, the appearance of 323.15K-393.15K hydrated aluminum oxide residue is earlier than the equilibrium of reaction 4; when pH = 5, the appearance of 300.15K-393.15K hydrated aluminum oxide residue is earlier than the equilibrium of reaction 4; when pH = 6-7, the appearance of 273.15K-393.15K hydrated aluminum oxide residue is earlier than the equilibrium of reaction 4.

5. The method according to claim 4, characterized in that In the temperature range of 273.15K-393.15K and pH=1-7, no kaolinite precipitation occurs during the 4-phase equilibrium period or the appearance of hydrous aluminum oxide residues.

6. The method according to claim 3, characterized in that When the temperature is higher than 393.15K, reaction 3 reaches equilibrium first. In the low temperature and low pH fluid environment, the reaction is more likely to develop spontaneous quartz precipitation before the equilibrium of reaction 3. As the pH value of the solution increases, the temperature range for the preferential appearance of quartz precipitation decreases: when pH = 1, 393.15K-548.15K; when pH = 2, 393.15K-513.15K; when pH = 3, 393.15K-468.15K; when pH = 4, 393.15K-438.15; when pH = 5, 393.15K-413.15K. Quartz precipitation already exists when reaction 3 reaches equilibrium. In other pH and temperature ranges, no quartz minerals precipitate before reaction 3 equilibrium; When pH = 1, 513.15K-593.15K; when pH = 2, 423.15K-593.15K; when pH = 3, 543.15K-623.15K; when pH = 4, 393.15-543.15K; when pH = 5, 393.15-483.15K; when pH = 6, 393.15-443.15K; when pH = 7, 373.15-403.15K; it is manifested as the preferential precipitation of boehmite before reaction 3 reaches equilibrium.

7. The method according to claim 6, characterized in that There was no kaolinite precipitation before the equilibrium of reaction 3, quartz precipitation and hydrous aluminum oxide residue.

8. The method according to claim 2, characterized in that Under the silica release model, the transformation pathways of albite particles in an acidic fluid environment include: Path A: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → reaction 2 and reaction 3 proceed simultaneously → reaction 2 and reaction 3 proceed simultaneously, quartz precipitates → reaction stops; Path B: Reaction 2, Reaction 3, Reaction 4, and Reaction 5 proceed simultaneously → Reaction 2 and Reaction 3 proceed simultaneously → Reaction 2 and Reaction 3 proceed simultaneously, quartz precipitation → Reaction 2 proceeds, quartz precipitation reaction → stops; Path C: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously, quartz precipitation → Reaction 2, reaction 3, and reaction 4 proceed, quartz precipitation → Reaction 2, quartz precipitation → reaction stops; Path D: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously, quartz precipitation → Reaction 2, quartz precipitation → reaction stops; Path E: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → reaction 2, reaction 3, and reaction 4 proceed simultaneously → reaction 2 proceeds → reaction 2, quartz precipitation → reaction stops; Path F: Reaction 2, Reaction 3, Reaction 4, and Reaction 5 proceed simultaneously → Reaction 2 proceeds → Reaction 2, quartz precipitation → reaction stops; Path G: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously, quartz precipitates → Reaction 2 proceeds, quartz precipitates → reaction stops; Path H: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2 proceeds → Reaction 2 proceeds, quartz precipitates → Reaction stops; Path I: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously → Reaction 2 proceeds → Reaction 2 proceeds, quartz precipitates → Reaction stops; Path J: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed → Reaction 2, reaction 3, and reaction 4 proceed together → Reaction 2 and reaction 3 proceed together → Reaction 2 and reaction 3 proceed together, quartz precipitates → Reaction 2 proceeds, quartz precipitates → reaction stops; Path K: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously → Reaction 2 and reaction 3 proceed simultaneously, quartz precipitates → reaction stops; Path L: Reaction 2, reaction 3, reaction 4, and reaction 5 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously → Reaction 2, reaction 3, and reaction 4 proceed simultaneously, and quartz precipitates → Reaction 2 proceeds, and quartz precipitates → the reaction stops.

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