Experimental Study on Corrosion Performance of Oil Tubing Steel in HPHT Flowing Media Containing O₂ and CO₂

Abstract

The high pressure and high temperature (HPHT) flow solution containing various gases and Cl⁻ ions is one of the corrosive environments in the use of oilfield tubing and casing. The changing external environment and complex reaction processes are the main factors restricting research into this type of corrosion. To study the corrosion mechanism in the coexistence of O₂ and CO₂ in a flowing medium, a HPHT flow experiment was used to simulate the corrosion process of N80 steel in a complex downhole environment. After the test, the material corrosion rate, surface morphology, micromorphology, and corrosion product composition were tested. Results showed that corrosion of tubing material in a coexisting environment was significantly affected by temperature and gas concentration. The addition of O₂ changes the structure of the original CO₂ corrosion product and the corrosion process, thereby affecting the corrosion law, especially at high temperatures. Meanwhile, the flowing boundary layer and temperature changed the gas concentration near the wall, which changed the corrosion priority and intermediate products on the metal surface. These high temperature corrosion conclusions can provide references for the anticorrosion construction work of downhole pipe strings.

1. Introduction

The thermal recovery technology of heavy oil, which is applied to the production of tight and shale oil in the oil field, has the characteristics of high construction temperature, complex flowing medium, and strong corrosiveness. Generally, the production process contains a variety of anions and cations and multicomponent gases, with temperature higher than 150 °C. As the only channel for oil or gas exploitation, the downhole tubing string is inevitably corroded by the high pressure, high temperature, and complex flowing solution, which cause deformation and fracture damage of tubing string, thereby affecting well site safety [1].

N80 tubing steel, which is commonly used in thermal recovery wells, is damaged by the corrosion of O₂, CO₂, and H₂S in the liquid containing HCO₃⁻, Cl⁻, SO₄²⁻, Ca²⁺, Mg²⁺, and Na⁺ [2]. The corrosion in the high temperature flowing liquid environment where O₂, CO₂, and Cl⁻ coexist is the focus of intense research for N80 tubing steel. The essence of the CO₂ corrosion for tubing steel is the electrochemical corrosion of metals in aqueous carbonate solution [3]. Thus, many studies have investigated CO₂ corrosion based on these factors. Bai et al. [4] investigated the influence of CO₂ partial pressure on the properties of J55 carbon steel in 30% crude oil/brine at 65 °C. The corrosion rate significantly increases as the CO₂ partial pressure increases from 0 to 1.5 MPa and decreases from 1.5 to 5 MPa, and the surface of J55 carbon steel is covered by FeCO₃ and CaCO₃. The CO₂ partial pressure changes the system pH and CO₂ solubility in crude oil, which further affects the formation and protection performance of the corrosive film. Zhang et al. [5] studied the corrosion behavior of N80 carbon steel under dynamic supercritical CO₂ (8 MPa)–water environment. The results demonstrated no essential difference in the electrochemical corrosion mechanism between supercritical CO₂ and nonsupercritical CO₂ (5 MPa) environments. The corrosion rate under dynamic condition is higher than that under static condition in the initial time and flowing fluid hinders the formation of corrosive film and then increases the corrosion rate.

De Waard et al. [6] studied the reaction process of the anode and cathode through the point-position mechanical polarization curve, and the anode reaction formula (Fe → Fe²⁺ + 2e⁻) containing OH⁻ was obtained. Nesic et al. [7] divided the pH value of the solution into PH < 4, 4 < PH < 6, and PH > 6; for the CO₂ anode electrochemical corrosion reaction process, an intermediate product Fe(CO₃)OH might be generated. Linter et al. [3] reported that Fe(OH)₂ occurs first in the process of CO₂ corrosion, and then FeCO₃ would be further generated. The CO₂ corrosion rate is generally controlled by the reaction of the cathode. Scholars locally and internationally have conducted many studies on cathode corrosion. The results showed that the corrosion rate of steel in CO₂ solution is controlled by H evolution kinetics [8].

O₂ is a catalyst for CO₂ corrosion and is also a cathodic depolarizer in the corrosion process of steel. When the protective film is not formed on the carbon steel surface, the corrosion rate will increase with the O₂ content, while the CO₂ content plays a decisive role in the corrosion of carbon steel after the O₂ content reaches saturation in solution. Once the protective film is formed on the surface, the corrosion of carbon steel is not affected by the O₂ content [9]. In the presence of O₂, a double-layer film structure is present in the CO₂ corrosive system, the inner of which is mainly Fe₂O₃, and the outer is the loose and porous corrosion product FeCO₃ [10]. The increase in O₂ content will result in a dense outer layer of corrosion product film to protect the steel surface. Another study [11] has found that the corrosion products on the 3Cr steel surface are formed by the accumulation of granular products under high temperature conditions where O₂ and CO₂ coexist, and the outer corrosion scales are mainly FeCO₃ and Fe oxides.

The influence of Cl⁻ is reflected in two aspects, as follows [12]: (1) the possibility of passivation film formation on the sample surface is reduced, or the damage of the passivation film is accelerated; therefore, the local corrosion reaction is promoted. (2) The solubility of CO₂ in the aqueous solution is reduced, which could alleviate the corrosion of carbon steel. The corrosion product film on the surface of N80 steel is denser, and the adhesion is high at a low Cl⁻ content (5000 mg/L), which indicates that corrosion resistance is improved [13]. When the Cl⁻ content increases twofold, the protective effect of the corrosive film decreases due to the weak compactness of the corrosive film, thereby resulting in an accelerated corrosion rate of steel. Some studies have compared the effects of Cl⁻ concentration and CO₂ concentration on the corrosion of carbon steel. The test results of Wang et al. [14] showed that the corrosion rate of N80 steel in 1–3 wt% NaCl solution is the highest. Meanwhile, there is a critical partial pressure of CO₂ in the chloride-containing solution that affects the corrosion rate. Zhang et al. [15] tested the corrosion law of N80 steel under different CO₂ partial pressures in detail. The results show that the increase in CO₂ partial pressure accelerates the corrosion reaction but, at the same, time forms a dense protective layer. However, in a chloride-containing solution, Cl⁻ is sufficient to penetrate the protective layer and react with the base metal [16].

High-pressure and high-temperature (HPHT) multicomponent media are the most common corrosion environments for N80 steel underground. To study the corrosion law of pipes, we used a high-temperature and high-pressure reactor to create an HPHT flow solution to simulate the corrosion environment. The corrosion rate, surface morphology, surface composition, and corrosion layer profile morphology results were obtained in the test. Meanwhile, the N80 corrosion process in an environment of coexisting CO₂ and O₂ has been discussed in various ways.

2. Experimental

2.1. Experimental System

The HPHT corrosion system was used for the flow-induced corrosion test of the N80 steel, including the HPHT autoclave (Weihai Global Chemical Machinery MFG Co., Ltd., Weihai, China), the lifting platform, the control cabinet, the booster pump, and the air source. As shown in Figure 1, the inside of the autoclave was made of Hastelloy C-276, which can resist corrosion under most conditions. The exterior of the autoclave is made of 304 stainless steel. The samples were installed on the fixture and rotated with the agitator shaft and fixture. Approximately 5 L of mixed fluid (simulated produced fluid in oilfield) was injected into an autoclave and stirred by an agitator. The dissolved oxygen was purged in the solution with injected nitrogen gas for 4 h under a pressure of 0.5 MPa. The autoclave was pressured with pure N₂ to the experimental values (total pressure value and CO₂ partial pressure) with CO₂ gas to the experimental values for 72 h at the flow velocity of 1 m/s. The surface microstructure of the corrosion product scales on the surface of the corroded samples was analyzed by JSM-6390 SEM (JEOL, Tokyo, Japan). The composition of the corroded samples was performed by XRD (LabX XRD-6000, SHIMADZU Co., Ltd., Kyoto, Japan).

2.2. Experimental Conditions

The composition of the experimental material, N80 tubing steel, is listed in

Table 1. Chemical composition of N80 steel (wt%).

Materials	C	Si	Mn	P	S	Cr	Mo	Ni	Cu	Fe
N80	0.22	0.21	1.77	0.01	0.003	0.036	0.021	0.028	0.019	97.683

. The samples were machined to dimensions of 50 × 13 × 1.5 mm. Before the experiment, the samples were placed in acetone to remove the surface oil and sequentially polished with 500#, 800#, 1200#, and 2000# sandpaper. The samples were scrubbed two times with distilled cotton in distilled water and cleaned for 15 s with distilled water. The samples were dried in cold air and placed in the dryer for 24 h. Finally, the samples were weighed using a digital balance with an accuracy of 0.1 mg.

After the experiment, the corroded samples were photographed to record the surface variations and then immersed in an acid solution (500 mL of HCl and 3.5 g hexamethylenamine diluted with water to 1000 mL) for 10 min to remove product films [4]. The samples were placed on absolute ethanol for washing two times until the acid cleaning solution on the surface was completely removed. The samples were dried and weighed before the test. When testing XRD, the product film of the sample was peeled off, and the crystal grain was ground to 0.1–10 μm. These grains were filled into the material tray and pressed to make the surface flat.

The volume of the produced liquid used in each set of experiments was 5 L, and the liquid ingredients are listed in

Table 2. Composition of test solution used in corrosion experiments.

HCO3− (mg/L)	Cl− (mg/L)	Ca2+ (mg/L)	Na+ (mg/L)	SO42− (mg/L)	Salinity (mg/L)	pH
800	2000	10	1785	400	4995	7.8

. The total pressure of HPHT corrosion was 5 MPa. The experimental temperature varied from 50 to 200 °C, and the solution flow velocity was fixed at 1 m/s. The CO₂ partial pressures were 0.25, 0.50, and 0.75 MPa, and the O₂ partial pressures were adjusted to 0.05, 0.10, and 0.15 MPa, respectively.

3. Results

3.1. Effects of Solution Temperature and CO₂ Partial Pressure on Corrosion Rate

The corrosion rate of N80 steel measured by changing the CO₂ concentration and temperature in the CO₂–O₂ coexisting environment (0.25 MPa CO₂ and 0.05 MPa O₂) is shown in Figure 2and Figure 3. The results show that the corrosion rating of N80 steel in this condition is severe or extremely severe according to the NACE SP 0775-2013 standard. When the partial pressure of CO₂ is 0.25 MPa, the corrosion rate increases with increasing temperature. When the partial pressure of CO₂ is greater than 0.5 MPa, the corrosion rate will have a maximum value at 100 °C with the increase in temperature. A comparison of the corrosion rate at different CO₂ partial pressures is shown in Figure 3. As the temperature increases, corrosion rate varies directly with CO₂ partial pressure at a temperature less than 100 °C and inversely at a temperature higher than 100 °C. This result indicates that the increase in CO₂ concentration at low temperature promotes the corrosion reaction, whereas the change in CO₂ concentration at high temperature weakens the effect of corrosion.

3.2. Macroscopic Morphology and Product Components

Figure 4 shows the surface morphology of N80 steel after corrosion at different temperatures in an O₂ and CO₂-containing environment. The results show that thick corrosion products are attached to the surface of the corroded material, which causes the metal matrix to be completely covered by precipitated scales. The product films on the surface are loose and thick, and a portion of them falls off at 50 and 100 °C. As the temperature increases from 100 to 200 °C, the product films become thin and smooth, and the color changes from deep red to black. The morphology of N80 steel after corrosion in a high-temperature environment containing 0.05 MPa O₂ by changing the partial pressure of CO₂ is shown in Figure 5. When the partial pressure of CO₂ is 0.25 MPa, the dark-brown corrosion surface is relatively flat, and a loose corrosion product film is attached. No hard scale is present on the surface of the corroded sample because the solubility of CO₂ will decrease at 200 °C. When the partial pressure of CO₂ reaches 0.75 MPa, the surface oxide of the material increases, and the product film thickens.

The SEM morphology and XRD test results of corrosion products of N80 steel in an environment of coexisting CO₂–O₂ at different temperatures are shown in Figure 6. The results show that the corrosion product film thickness is mainly composed of FeCO₃ and Fe₂O₃ at 50 °C. The granular products on the surface are wrapped in the corrosion layer at 100 °C, which causes the surface of the sample to be uneven. The corrosion products are mainly composed of FeCO₃, Fe₂O₃, and Fe₃O₄. Fe₂O₃ is oxidized again to Fe₃O₄ at 150 °C, which increases the particle attachment. When the temperature continues to increase to 200 °C, the product structure on the surface of the material is stable and dense.

The SEM morphology and XRD test results of corrosion products of N80 steel at different CO₂ partial pressures are shown in Figure 7. The SEM result with a CO₂ partial pressure of 0.25 MPa shows that the corrosion products on the surface layer are relatively thin and have not been connected to form an overall structure. When the partial pressure of CO₂ increases to 0.5 MPa, the product film falls off significantly, and large corrosion cracks appear on the surface. The iron oxides completely cover the original corrosion products to form a double-layer film structure on the surface in a high-concentration CO₂ environment (P_CO2 = 0.75 MPa). This kind of membrane structure is not dense or unstable and is easily washed off by the solution, which causes the internal matrix to continue to corrode. The XRD measurement results of the corrosion product of the material show that the surface of the corroded material is covered with FeCO₃ grains and iron oxides because when the corrosive environment contains CO₂ and O₂, FeCO₃ and Fe(OH)₂ corrosion product films will appear on the initial surface, and then O₂ in the environment will oxidize with Fe(OH)₂ and FeCO₃ to form iron oxides [3,7]. The corrosion products on the final surface are mainly iron oxides, such as FeCO₃, Fe₂O₃, and Fe₃O₄. The outer layer of the formed double layer corrosion product film is mainly composed of FeCO3 and Fe oxides, while the inner layer is mainly composed of regular grained FeCO₃. Compared with a single CO₂ corrosion product, the appearance of oxides reduces the integrity of the corrosion product film and increases the corrosion rate of the material.

Figure 8 shows the surface structure after removing the outer layer of the attached product film. The corrosion surface is composed of small corrosion pits that are connected to uneven honeycomb areas at 50 °C. At 100 and 150 °C, the corroded surface is spliced by a large area of massive corrosion pits. The original corrosion products are composed of flaky structures due to the gradual expansion of the local fine pits to form a certain area, and the corrosion products gradually accumulate to form a layer. Under the action of liquid shearing force, the flaky corrosion products on the surface of the material fall off to form a large uneven area. Deep corrosion pits appear on the film surface at 150 °C, and a small amount of corrosion product is mixed in the corrosion pits. This result indicates that the flowing liquid penetrated into the material matrix through the cracks, which causes serious pitting corrosion in the internal surface. The surface of the material is relatively regular and smooth without evident pitting after corrosion at 200 °C, and the corrosion products are mainly flakes.

Figure 9 shows the cross-sectional morphology of the corrosion sample. According to different positions, the sample surface can be divided into an adhesion layer, corrosion layer, and matrix. Among these layers, the adhesion layer is the loosest and consists of crystalline particles or oxide. The corrosion layer is mainly formed by the accumulation of reaction intermediate products and dense corrosion product. The corrosion layer is not enough to prevent macromolecules and ions from contacting the metal surface, especially in flowing liquids, because it contains large pores. For the same reason, the corrosion layer is a porous medium, which cannot prevent Cl ions from contacting the substrate. Hence, when the temperature is in the range of 100 to 150 °C, serious continuous corrosion pits appear in the corrosion layer and extend to the depths of the matrix.

4. Discussion

Given that the total pressure in this experiment is 5 MPa, according to the law of O₂ and CO₂ gas saturation pressure changing with temperature, the fluid in the kettle is in the form of gas–liquid coexistence at this experimental temperature. During the rotation of the sample, the surface of the material is subjected to the fluid shear force, which accelerates the rupture of the corrosion product film. Meanwhile, the rapid fluid flow accelerates the convective mass transfer of the gas in the boundary layer of the sample surface, thereby changing the corrosion process. According to the characteristics shown by the experimental results, the main factor affecting the corrosion of N80 in the high-temperature and high-pressure flowing media is the change in the reaction of O₂ or CO₂ under different flow velocities and temperatures.

4.1. Formation of Corrosive Environment Containing CO₂

The essence of the corrosion of CO₂ and steel materials is the electrochemical reaction of metals in carbonic acid solution. Although the carbonic acid produced by dissolving CO₂ in water is a dibasic acid, the acidity of carbonic acid is higher than that of hydrochloric acid under the same pH value, which will cause serious corrosion to steel materials. Nesic [7] divided the pH value of the solution as follows: pH < 4, 4 < pH < 6, and pH > 6. Nesic believes that Fe(CO₃)OH intermediate products can be generated during the electrochemical reaction of the anode. Thus, the anode reaction is as follows:

$$\begin{gathered} \mathrm{p}\mathrm{H}<4 \\ {\mathrm{H}}_3{\mathrm{O}}^{+}+{\mathrm{e}}^{-}\to \mathrm{H}+{\mathrm{H}}_2\mathrm{O}, \end{gathered}$$

(1)

$$\begin{gathered} 4<\mathrm{p}\mathrm{H}<6 \\ {\mathrm{H}}_2{\mathrm{CO}}_3+{\mathrm{e}}^{-}\to \mathrm{H}+{\mathrm{HCO}}_3^{-}, \end{gathered}$$

(2)

$$\begin{gathered} \mathrm{p}\mathrm{H}>6 \\ {2\mathrm{HCO}}_3^{-}+2{\mathrm{e}}^{-}\to {2\mathrm{H}}_2{+2\mathrm{CO}}_3^{2-}, \end{gathered}$$

(3)

Moreover, the overall reaction equation is as follows:

$${\mathrm{Fe}+\mathrm{CO}}_2{+\mathrm{H}}_2\mathrm{O}\to {\mathrm{FeCO}}_3{+\mathrm{H}}_2$$

(4)

In this experiment, the pH of several groups of media is between 4 and 6. As shown in Figure 10, the CO₂ corrosion rate decreases with increasing temperature. Therefore, when the temperature is less than 100 °C, a H depolarization process exists in the electrochemical reaction. The process is completed by HCO₃⁻ and H⁺, which are decomposed by H₂CO₃ in the solution. The higher the partial pressure of CO₂ is, the higher the solubility of H₂CO₃ is, and the higher the H⁺ concentration produced by the hydrolysis of H₂CO₃ in the solution will be, thereby resulting in fast corrosion of the material [17,18]. However, in a high-temperature environment (T > 150 °C), the decrease in the solubility of CO₂ and increase in pH of the solution reduce the anode reaction rate. Therefore, the corrosion rate increases with the increase in CO₂ concentration at low temperature but decreases at high temperature.

4.2. Diffusion and Reaction of O₂ in CO₂ Solution

The results of comparing the corrosion rate of N80 steel with and without O₂ are shown in Figure 11. In an environment containing only CO₂ gas, the surface corrosion rate of N80 shows a law that first increases and then decreases. When the temperature reaches 200 °C, the corrosion rate decreases to <0.5 mm/a. In an environment containing only O₂ gas, the corrosion rate increases with the increase in temperature, and the maximum corrosion rate occurs at 200 °C. When O₂ is added to the CO₂ corrosive medium, the corrosion rate is higher than that of a single gas environment. The corrosion ratio obtained by comparison is shown in Figure 12. When the CO₂ partial pressure is less than 0.5 MPa, the corrosion rate change law is similar to that of a single CO₂ environment. However, when the partial pressure of CO₂ is 0.75 MPa, the corrosion rate continues to increase with the increase in temperature, which indicates that the addition of O₂ significantly changes the CO₂ corrosion process in a high-concentration and high-temperature environment. Given that the flow velocity does not change, the forced convection flow in the boundary layer of the same phase medium is close. The results show that the corrosion contrast at different temperatures is significantly different, which indicates that the O₂ mass transfer law in the corrosion product film affects the electrochemical reaction of the substrate.

The diffusion and mass transfer of O₂ in the film restricts the rate of the depolarization reaction because the N80 surface forms a FeCO₃ film on the metal surface in the H₂CO₃ solution. In a steady-state mass transfer unit, dC/dt = 0, the total molar flux is defined by the Nernst–Plank equation, as follows [18]:

$$\mathrm{J}=-\mathrm{D}\frac{\mathrm{dC}}{\mathrm{dx}}-\frac{\mathrm{nFDC}}{\mathrm{RT}}\frac{\mathrm{df}}{\mathrm{dx}}{+\mathrm{Cv}=\mathrm{J}}_{\mathrm{d}}{+\mathrm{J}}_{\mathrm{m}}{+\mathrm{J}}_{\mathrm{c}}.$$

(5)

Take the corrosion of N80 steel in water at 150 °C and 5 MPa pressure as an example. According to the first boundary condition of Fick’s second law [19], the expression of reactant concentration at any position in the boundary layer is obtained as follows:

$$\frac{{\mathrm{C}}^{\mathrm{y}}{-\mathrm{C}}^{\mathrm{a}}}{{\mathrm{C}}^{\mathrm{w}}{-\mathrm{C}}^{\mathrm{a}}}=1-\mathrm{erf}(\frac{\mathrm{y}}{\sqrt{4\mathrm{Dt}}}),$$

(6)

$${\mathrm{C}}^{\mathrm{y}}{=\mathrm{C}}^{\mathrm{w}}{-(\mathrm{C}}^{\mathrm{w}}{-\mathrm{C}}^{\mathrm{a}}\left)\mathrm{erf}\right(\frac{\mathrm{y}}{\sqrt{4\mathrm{Dt}}}),$$

(7)

where the erf(y) is the error function, and the O₂ concentration in the water is approximately equal to 0.044 mol/L [20]. According to the diffusion layer thickness formula δ = (πDt)^0.5, the calculated boundary layer thickness when O diffuses for 1 s is 0.08 mm. Therefore, three positions near the wall—that is, y = 0.05 mm, diffusion layer interface y = 0.1 mm, and outside the diffusion layer y = 0.15 mm—are taken to calculate the change in O concentration C^y. As shown in Figure 13, when the wall surface O concentration was 1/10 of the diffusion outer layer concentration, the O molecules participating in the electrochemical cathode reaction accounted for 90% of the total molecules. The O concentration in the diffusion layer (x = 0.05 mm) significantly decreases with time—that is, approximately 38% in 1 s. Meanwhile, the diffusion layer interface (x = 0.1 mm) only decreases by 10%. This result shows that in the film, within a short time of the formation of the electrochemical system, the concentration of the reactants forms a larger concentration gradient in the diffusion layer because the oxygen content that is involved in the reaction accounts for 90%, the electrochemical reaction is rapid, and the system is controlled by the reactant concentration.

According to the solubility of O₂ and CO₂ in water at different temperatures tested by Duan and Broden [20,21], as shown in

Table 3. Solubility of O₂ and CO₂ in water under 5 MPa pressure (mol/L) [20,21].

	T (°C)	50	60	90	100	120	130	150	210
Gas
O2		0.044	—	—	0.036	—	0.038	0.044	—
CO2		—	0.669	0.495	—	0.415	—	0.377	0.299

, the solubility of CO₂ in water is 10- to 20-fold higher than that of O₂ at temperatures ranging from 50 to 200 °C. This result shows that CO₂ derived more reactants than O₂ in a high-temperature environment. However, under the coexistence of O₂ and CO₂, O₂ first combines with Fe²⁺ or Fe³⁺ to form Fe(OH)₃ (Equations (8) and (9)) because O₂ oxidizes more than H₂CO₃ and H⁺. A part of Fe²⁺ can combine with HCO³⁻ to form FeCO₃ crystals (Equation (10)). In a high-temperature environment, Fe(OH)₃ and FeCO₃ are decomposed into Fe₂O₃, which has poor adhesion and poor ability to form a film, as shown in Equations (11)–(13).

$$\begin{gathered} \mathrm{First\; reaction\; stage} \\ {4\mathrm{Fe}}^{2+}{+4\mathrm{H}}^{+}{+\mathrm{O}}_2\to {4\mathrm{Fe}}^{3+}{+2\mathrm{H}}_2\mathrm{O}, \end{gathered}$$

(8)

$$\begin{gathered} \mathrm{First\; reaction\; stage} \\ {\mathrm{Fe}}^{3+}{+3\mathrm{H}}_2\mathrm{O}\to {\mathrm{Fe}\left(\mathrm{OH}\right)}_3{+3\mathrm{H}}^{+}, \end{gathered}$$

(9)

$$\begin{gathered} \mathrm{First\; reaction\; stage} \\ {\mathrm{Fe}}^{2+}{+\mathrm{HCO}}_3^{-}\to {\mathrm{FeCO}}_3{+\mathrm{H}}^{+}+2\mathrm{e}, \end{gathered}$$

(10)

$$\begin{gathered} \mathrm{Second\; reaction\; stage} \\ {\mathrm{Fe}\left(\mathrm{OH}\right)}_3\to {\mathrm{FeO}\left(\mathrm{OH}\right)+\mathrm{H}}_2\mathrm{O}, \end{gathered}$$

(11)

$$\begin{gathered} \mathrm{Second\; reaction\; stage} \\ 2\mathrm{FeO}\left(\mathrm{OH}\right)\to {\mathrm{Fe}}_2{\mathrm{O}}_3{+\mathrm{H}}_2\mathrm{O}, \end{gathered}$$

(12)

$$\begin{gathered} \mathrm{Second\; reaction\; stage} \\ {4\mathrm{FeCO}}_3{+\mathrm{O}}_2\to {2\mathrm{Fe}}_2{\mathrm{O}}_3{+4\mathrm{CO}}_2. \end{gathered}$$

(13)

In addition to the effect on the priority of the reaction on the metal surface, the penetration of O₂ into the product film will also affect the surface structure. As shown in Figure 14, local reactions occurred inside the product film because the FeCO₃ film was not enough to isolate O₂ molecules, and the liquid flow made the product film thin. When O₂ molecules enter the film, they will react with FeCO₃ to form Fe₂O₃ and CO₂, and a small amount of H₂ will be generated by the partial H evolution reaction. When gas accumulates inside, it will swell inside the product film and eventually break the film. The flow of external liquid will also accelerate the rupture of the corrosion film.

4.3. Influence of Temperature

In addition to the influence of mass transfer, reaction priority, and reaction position on the corrosion of N80 in the coexisting environment, temperature also changes the progress and rate of several reactions. First, temperature will affect the corrosion process dominated by chemical reactions and the dissolution and diffusion of CO₂/O₂ in the solution. Second, temperature will affect the oxidation of Fe²⁺, the deposition of corrosion product FeCO₃, and the formation of corrosion intermediate products. These factors increase the complexity of the corrosion process and surface characteristics of the material.

Temperature can affect the gas dissolution and diffusion rate and further affect the composition, compactness, and corrosion rate of the corrosion product film of N80 steel in the CO₂–O₂ environment. As shown in Figure 2, when the partial pressures of CO₂ are 0.50 and 0.75 MPa, and the temperature is less than 50 °C, the slow diffusion rate of O₂ causes the surface corrosion of the material to be dominated by CO₂ corrosion. When the temperature continues to increase and is less than 150 °C, part of the FeCO₃ film will be transformed into Fe₂O₃. At this time, the corrosion rate increases because Fe₂O₃ is loose and easily falls off. Meanwhile, due to changes in the structure of the corrosion product film, a part of the corrosion product film is easily penetrated by O₂ and Cl⁻. Fe ions can also diffuse into the solution through the microporous structure on the corrosion product film, which accelerates the dissolution of iron. When the temperature is higher than 150 °C, several iron oxides become dense and protective, and the corrosion rate will decrease.

5. Conclusions

To study the corrosion law of tubing materials in HPHT flowing media, corrosion experiments were carried out in a test liquid containing O₂ and CO₂. According to the corrosion rate, corrosion morphology, and product composition obtained by the experiments, the following conclusions can be drawn.

(1) When the CO₂ concentration was low in the coexistence environment, the corrosion rate of N80 was affected by O₂ and continued to increase with increasing temperature. When the CO₂ concentration increased (when the volume fraction was higher than 10%), the corrosion rate had a maximum value near 100 °C.

(2) O₂ and temperature affected the changes in intermediate products and film structure of the CO₂ corrosion. The oxide formed by the reaction of O₂ and Fe will cover the surface of regular FeCO₃ grains, which may destroy the original single structure of the product film and cause the surface film to rupture or form cracks. The temperature increase will also accelerate the rupture process.