The Corrosion Behavior of Pure Iron under Solid Na₂SO₄ Deposit in Wet Oxygen Flow at 500 °C

Abstract

The corrosion behavior of pure Fe under a Na₂SO₄ deposit in an atmosphere of O₂ + H₂O was investigated at 500 °C by thermo gravimetric, and electrochemical measurements, viz. potentiodynamic polarization, electrochemical impedance spectroscopy (EIS), and surface characterization methods viz. X-ray diffraction (XRD), and scanning electron microscope (SEM)/energy dispersive spectroscopy(EDS). The results showed that a synergistic effect occurred between Na₂SO₄ and O₂ + H₂O, which significantly accelerated the corrosion rate of the pure Fe. Briefly, NaFeO₂ was formed in addition to the customary Fe oxides; at the same time, H₂SO₄ gas was produced by introduction of water vapor. Subsequently, an electrochemical corrosion reaction occurred due to the existence of Na₂SO₄, NaFeO₂, and H₂O. When this coupled to the chemical corrosion reaction, the progress of the chemical corrosion reaction was promoted and eventually resulted in the acceleration of the corrosion of the pure Fe.

1. Introduction

In the last decade, it has been found that the corrosion of some pure metals and their alloys such as 1Cr11NiW2MoV, Fe-5Cr, Fe-15Cr, and Fe-25Cr (mass percent) was accelerated under solid NaCl in an atmosphere of H₂O + O₂ at intermediate temperatures (300–600 °C) [1,2,3,4,5,6,7,8]. This phenomenon has been notably reflected in the corrosion of turbine blades in aeroplanes serving in the vicinity of the sea. Actually, a synergistic effect, which is prone to accelerate the corrosion of metals/alloys, was observed when solid salt such as NaCl and water vapor (H₂O) were used together at 300–600 °C [1,2,3,4,5,6,7,8]. Shu et al. [1,2,3,4] found that the involvement of H₂O significantly accelerated the corrosion rate of many pure metals and alloys. This is especially the case for pure Cr. Based on this observation, many researchers considered that there might be some electrochemical reactions related to the corrosion process. One of the possible explanations is that H₂O continuously evaporates and subsequently absorbs on the layer of salt [1], which promotes the electrochemical reactions and eventually accelerates the metal s corrosion [2]. However, the mechanism has not yet been confirmed by experiment. To understand the mechanism, firstly, electrochemical measurements including cell testing, use of electrodes, and electrochemical impedance spectroscopy (EIS) were set up by the authors and used to study the electrochemical behavior, which confirmed that the electrochemical reactions occurred during the corrosion of pure Fe under a solid NaCl deposit in a water vapor atmosphere [9]. In addition, the co-reaction between electrochemical and chemical reactions was observed, which confirmed that the corrosion of the metals was accelerated under the salt deposit in the atmosphere of H₂O + O₂. However, the corrosion mechanism (i.e., the corrosion reaction) has not yet been studied in detail and further effort is required.

The deposit of sulfates (especially Na₂SO₄) on metallic parts which operate under damp air at intermediate or high temperatures is a normal phenomenon, such as occurs with gas turbines and power plants located in marine environments [8]. According to previous studies [1,2,3,4,5,6,7,8], a co-effect between deposited sulfate and H₂O + O₂ might exist and significantly accelerate the corrosion of metals in a similar way to that occurring with NaCl + H₂O + O₂. However, studies on the synergistic effects of Na₂SO₄ + H₂O + O₂ on the corrosion of metals or alloys are still lacking. Based on the operating temperature, the sulfate deposit has two different forms, molten and solid. Recently, many studies have been carried out on the corrosion behavior of metals/alloys in a molten Na₂SO₄ environment [10,11,12,13,14,15,16] and many corrosion mechanisms have been proposed. One of the well-known mechanisms is the sulfidation model [10,11], in which the formation of sulfides accelerates the corrosion. The other one is the acidic-basic fluxing [10,12,13,14,15] mechanism, in which dissolution of the scale of protective oxides due to formation of basic Na₂O was considered as the reason for the accelerated corrosion. Moreover, based on the electrochemical mechanism [16], corrosion was considered as an electrochemical reaction in which the transfer of electrons accelerated the corrosion. However, the corrosion mechanism under a solid sulfate deposit at an intermediate temperature (~500 °C) has not yet been widely investigated, without which the development of protection methods for metals or alloys has been restricted.

In order to reveal the corrosion mechanisms of the turbine blades in aeroplanes and ships straightforwardly, the pure metal was used for simplification. In previous studies, the corrosion behavior of pure Fe and Cr under solid NaCl in wet oxygen was studied, which showed a faster corrosion rate compared to only NaCl or wet oxygen alone. However, the effect of solid Na₂SO₄ in wet oxygen on stainless steel has not been studied before. Therefore, this work focuses on the corrosion behavior of metals under solid Na₂SO₄ in wet oxygen. Normally, the material used for turbine blades in aeroplanes is 1Cr11NiW2MoV steel, in which Fe is a main component. To study the corrosion mechanisms of the pure metal, it is helpful to understand the corrosion behavior of the turbine blades. The main metals in stainless steel are Fe and Cr. Both of these metals need be studied in detail. In this paper, the corrosion behavior of pure Fe under solid Na₂SO₄ deposit in an atmosphere of water vapor plus oxygen was investigated firstly by mass gain measurement, EIS, X-ray diffraction (XRD), scanning electron microscope (SEM). The corrosion mechanism is discussed in detail.

2. Results

2.1. Mass Gain Measurements

Figure 1 shows the mass gain of the pure Fe as a function of time at 500 °C in four different corrosion environments: (I) dry O₂; (II) H₂O + O₂; (III) Na₂SO₄ + O₂; and (IV) Na₂SO₄ + H₂O + O₂. As can be seen from Figure 1, the mass gain of the pure Fe under the different environments shows an increasing order of IV < I < II < III, which implies that a Na₂SO₄ deposit could inhibit the oxidation process of the pure Fe under certain conditions, particularly in the absence of H₂O. The highest mass gain was observed when H₂O + O₂ was introduced together with Na₂SO₄, which suggests that a synergistic effect exists between Na₂SO₄ and H₂O + O₂ on the corrosion process of the pure Fe, which accelerates the corrosion of the pure Fe at 500 °C.

Figure 1. Corrosion kinetics curves of the pure Fe under various corrosion environments at 500 °C: (I) dry O₂ (▲); (II) H₂O + O₂ (●); (III) Na₂SO₄ + O₂ (♦),and (IV) Na₂SO₄ + H₂O + O₂ (■).

Figure 1. Corrosion kinetics curves of the pure Fe under various corrosion environments at 500 °C: (I) dry O₂ (▲); (II) H₂O + O₂ (●); (III) Na₂SO₄ + O₂ (♦),and (IV) Na₂SO₄ + H₂O + O₂ (■).

2.2. Electrochemical Corrosion

Figure 2 shows the galvanic corrosion current (I_g) as a function of time for a couple of Fe-Pt under a solid Na₂SO₄ deposit with an atmosphere of H₂O + O₂ at 500 °C. The result shows that the I_g decreases from about 3 × 10⁻⁵ A/cm² to 1 × 10⁻⁵ A/cm² with an increase in time from 0 to 1200 s. Figure 3 shows the potentiodynamic polarization curves of the pure Fe under the testing environment. As can be seen, the anodic current density linearly increases with increases in the anodic potential in the active polarization zone, which can be attributed to the active dissolution of the metal. Figure 4 shows an in situ EIS result of the pure Fe after 1 h corrosion under the testing environment. It shows two time constants in the Nyquist plot. The capacitances correspond to the electrochemical reaction and the formation of oxidation products on the surface of the electrode at high and low frequencies, respectively [8]. Figure 5 shows the frequency dependence of the phase angle of the pure Fe with the Na₂SO₄ deposit and the H₂O + O₂ at 500 °C at open circuit potential. Figure 6 shows the cathodic potential dependence of the phase angle of the pure Fe under the Na₂SO₄ deposit and the H₂O + O₂ at 500 °C. As can be seen, the potential E corresponding to the maximum of cotΦ is negative to E_1/2 (semiwave potential).

Figure 2. Galvanic corrosion current of the Fe-Pt couple under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C.

Figure 2. Galvanic corrosion current of the Fe-Pt couple under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C.

Figure 3. The potentiodynamic polarization plot of the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C.

Figure 3. The potentiodynamic polarization plot of the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C.

Figure 4. EIS measurement results of the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ after 1 h oxidation at 500 °C: (A) Nyquist plot; (B) Bode plot.

Figure 4. EIS measurement results of the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ after 1 h oxidation at 500 °C: (A) Nyquist plot; (B) Bode plot.

Figure 5. Frequency dependence of the phase angle of the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C at open circuit potential.

Figure 5. Frequency dependence of the phase angle of the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C at open circuit potential.

Figure 6. Cathodic potential dependence of the phase angle of the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C.

Figure 6. Cathodic potential dependence of the phase angle of the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C.

2.3. Corrosion Products and Morphologies

After corrosion tests, the samples were analyzed by XRD after cleaning with distilled water. Figure 7 shows the XRD patterns of the corrosion scale formed on the surface of the Fe in the Na₂SO₄ + H₂O + O₂ environment after 10 h. The results show that the corrosion scale is composed of Fe₃O₄, Fe₂O₃, and NaFeO₂. Figure 8 shows an example of SEM surface morphology of the corroded sample with a deposited Na₂SO₄ layer in a H₂O + O₂ atmosphere at 500 °C after 10 h. It can be seen that the Na₂SO₄ layer turned from an originally thick and compact layer to a loose and porous one after 10 h. The corrosion scale with a bar-shape appears underneath the Na₂SO₄ layer. Obviously, Na₂SO₄ participates in the corrosion reaction of the pure Fe.

Figure 7. X-ray diffraction (XRD) results of the corrosion scale of the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C.

Figure 7. X-ray diffraction (XRD) results of the corrosion scale of the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C.

Figure 8. The morphology of the Na₂SO₄ film on the surface of the pure Fe after corrosion under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ for 10 h.

Figure 8. The morphology of the Na₂SO₄ film on the surface of the pure Fe after corrosion under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ for 10 h.

Figure 9 shows the SEM morphologies of the corrosion scale on the surface of the pure Fe after corrosion for 1 h and 10 h in the Na₂SO₄ + H₂O + O₂ environment at 500 °C after the Na₂SO₄ residual layer has been removed. The corrosion scale is uniform after corrosion for 1 h. The corrosion product is porous, which may be produced by the formation of volatile products [2]. However, the product scale changes to be uneven after corrosion for 10 h. In addition, the morphologies of needle- and nubbly-shape appear which are not seen in the case after 1 h. From the corresponding EDAX results (see Figure 10), the needle-shape product is composed of Fe, Na, and O elements, while Fe and O are the only two elements detected in the nubbly structure. According to the XRD and the previous research results [17], the needle-shape product is most likely a mixture of Fe₂O₃ and NaFeO₂ and the nubbly product may be Fe₃O₄. Figure 10 shows the cross-sectional morphologies of the corrosion scale on the pure Fe after corrosion for 1 h and 10 h under a Na₂SO₄ deposit in a H₂O + O₂ atmosphere at 500 °C. After 1 h, the layer of corrosion products is thin, porous, and cracked. After 10 h, the product scale is entirely different from that at 1 h, i.e., the outer part of the product scale has a lot of pores; the inner part of the scale is comparatively compact but has some micro-cracks.

Figure 9. Surface morphologies of the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ after different corrosion times: (A) 1 h; (B) 10 h.

Figure 9. Surface morphologies of the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ after different corrosion times: (A) 1 h; (B) 10 h.

Figure 10. Energy dispersive X-ray spectroscopy (EDAX) results of the products formed on the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ after corrosion for 10 h: (A) nubbly-shape products; and (B) needle-shape products.

Figure 10. Energy dispersive X-ray spectroscopy (EDAX) results of the products formed on the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ after corrosion for 10 h: (A) nubbly-shape products; and (B) needle-shape products.

3. Discussion

3.1. The Interaction between Electrochemical Corrosion Reaction and Chemical Corrosion Reaction

The galvanic corrosion current measurement reveals that the I_g of the coupled Fe-Pt under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C is about 10⁻⁵ A/cm² (Figure 3). It is believed that no electrochemical reaction occurs on Pt-Pt electrodes under the tested corrosion environment and its corresponding tested current density is near to zero [9]. Compared to the Pt-Pt electrodes, the appearance of current density in the Fe-Pt electrodes supplies the required information as it is produced by electrochemical reactions. Thus, electrochemical reactions are considered to be involved in the corrosion of the pure Fe under the tested environment. The entire corrosion reactions including the electrochemical corrosion reaction and the chemical oxidation reaction are the same as the results obtained under the solid NaCl deposit in an atmosphere of H₂O + O₂ at 600 °C [18]. The percentage of the electrochemical corrosion to the total corrosion was calculated, because it provides a useful insight into the corrosion behavior of the pure Fe under a solid Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C. The total corrosion rate can be calculated by mass gain measurements from the consumption of Fe over the entire corrosion. Since the oxidation products are mainly composed of the oxygen involved in the corrosion process and the metal consumed by corrosion, which is approximately Fe₂O₃, then the ratio of atoms is assured. The total amount of the consumed metal (Fe) can be determined from the mass gain results, which is calculated from the total Fe₂O₃ amount according to the ration of atoms. The electrochemical corrosion rates (I_corr) can be calculated by fitting the potentiodynamic polarization curves in the anodic active polarization zones. The calculation method is described in detail in the following reference [18]. In this study, the calculated percentage of the electrochemical corrosion to the total corrosion is about 1.4%, which is low and means the electrochemical corrosion is weak during the entire corrosion process.

In previous studies [9,18], the percentages of the electrochemical corrosion to the total corrosion of the pure Fe and the pure Cr are also small under a solid NaCl deposit in an atmosphere of H₂O + O₂ at intermediate temperature. However, the following study reveals that the electrochemical corrosion reaction couples to the preceding chemical corrosion reaction, which significantly accelerates the corrosion. According to the results, it is clear that the corrosion rate of the Fe under the environments of Na₂SO₄ alone, or H₂O alone, is significantly lower than that under both Na₂SO₄ + H₂O. The results show that with salt alone or H₂O alone, only the chemical reaction occurs [18]. While under the synergistic effect of salt and H₂O, the electrochemical and chemical reaction will co-effect on the corrosion [18]. Therefore, it can be concluded that the occurrence of the electrochemical corrosion reaction promotes the progress of the chemical corrosion reaction, which sharply accelerates the corrosion rates of the pure Fe and the pure Cr [18]. Also, from Figure 2, the corrosion rate of the pure Fe is dramatically accelerated under the solid Na₂SO₄ deposit in the water vapor, which implies that the corrosion rate of the pure Fe may be accelerated due to the introduction of an electrochemical corrosion reaction.

From the EIS results, the corresponding electrochemical parameters may be obtained. Among them, Φ is the phase angle and ω is the angle frequency [18]. It is well-know that different mathematic calculations for these parameters have different physical meanings. According to Smith [19], a plot of cotΦ vs. ω^1/2 can be used for mechanistic diagnosis. For example, an electrochemical reaction coupled to either a preceding chemical reaction (ce) or a following chemical reaction (ec) will show a maximum in a plot of cotΦ vs. ω^1/2, while a catalytic reaction (ec´) will give cotΦ close to infinity as ω is close to zero, where c´ is a catalytic reaction. If the electrochemical reaction does not couple to a chemical reaction, the plot of cotΦ vs. ω^1/2 will show a straight line. The frequency dependence of the phase angle of the pure Fe under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C at the open circuit potential is shown in Figure 5. The result shows that it is not a straight line and has a maximum. Therefore, the coupled effect of the electrochemical reaction and the chemical reaction can be confirmed.

However, the plot of cotΦ vs. ω^1/2 cannot be used to distinguish between these two mechanisms but the plot of cotΦ vs. (E − E_1/2) is required. For a chemical reaction in which the reaction rate constants k₁ = k₂, from the ce mechanism, the potential E corresponding to the maximum of cotΦ is negative to E_1/2; whereas for ec, the potential E corresponding to the maximum of cotΦ is positive to E_1/2. For a chemical reaction in which k₁ ≠ k₂, from the ce mechanism, the cotΦ decreases with increasing (E − E_1/2); whereas for an ec mechanism, the cotΦ increases with increasing (E − E_1/2) [19]. Figure 6 shows the cathodic potential dependence of the phase angle of the pure Fe under a Na₂SO₄ deposit in the atmosphere of H₂O + O₂ at 500 °C. The result indicates that the cotΦ increases with increasing (E − E_1/2), which means that corrosion mechanisms are consistent to the ce mechanism.

3.2. The Corrosion Behavior of the Pure Fe under a Na₂SO₄ Deposit in an Atmosphere of H₂O + O₂

The significantly increased corrosion rate of the pure Fe under a Na₂SO₄ deposit in the presence of H₂O suggests that the effect of H₂O on the corrosion is important and cannot be neglected. The formation of the corrosion scale with the porous layer (Figure 9A) may be due to the formation of volatile products during the corrosion process [8]. Figure 11 shows the cross-sectional morphologies of the corrosion products. The introduction of the H₂O may promote the formation of H₂ [20], which is one of the hypotheses that is not yet experimentally confirmed. However, the porous product scale confirms the formation of the volatile products. Based on this and previous study results [1,2,3,4,5,6,7,8,9,18], the following corrosion mechanism is proposed: at initial stages of the corrosion, the Na₂SO₄ and the H₂O can react with the Fe to produce NaFeO₂ and H₂SO_4(g):

4Fe + 3O₂ + 2H₂O +2Na₂SO₄ → 4NaFeO₂ + 2H₂SO₄(g)

(1)

Based on the above results and discussion as well as our previous study [9,17], in the electrochemical corrosion reaction coupled with a chemical corrosion reaction, the H₂SO₄ would electrochemically react with the Fe.

Cathodic reaction: H₂SO₄ + 2e^- → SO₄^2- + H₂

(2)

Anodic reaction: Fe − 2e^- → Fe²⁺

(3)

From these reactions, H₂SO₄ can be consumed by the cathodic reaction. Subsequently, the chemical reaction of (1) will be promoted in the forward direction. The electrochemical reaction can promote the progress of the chemical reaction, which will accelerate the corrosion rate of the pure Fe.

FeSO₄ can also react with the H₂O and the O₂ to form iron oxides and H₂SO₄(g) [6,8]:

6FeSO₄ + O₂ + 6H₂O → 2Fe₃O₄ + 6H₂SO₄(g)

(4)

5FeSO₄ + O₂ + 5H₂O → Fe₃O₄ + Fe₂O₃ + 5H₂SO₄(g)

(5)

The produced H₂SO₄(g) will cyclically react with the Fe, and continuously accelerate the corrosion process.

Meanwhile, during the corrosion process, the pure Fe would be oxidized by the following reactions by the H₂O and the O₂ in addition to the above mechanism [1]:

2Fe + 2H₂O + O₂ → 2Fe(OH)₂

(6)

6Fe(OH)₂ + O₂ → 2Fe₃O₄ + 6H₂O

(7)

Figure 11. Cross-sectional morphologies of the corrosion scale of the pure Fe under a Na₂SO₄ deposit in the atmosphere of H₂O + O₂ after corrosion for 1 h and 10 h.

Figure 11. Cross-sectional morphologies of the corrosion scale of the pure Fe under a Na₂SO₄ deposit in the atmosphere of H₂O + O₂ after corrosion for 1 h and 10 h.

3.3. Thermodynamic Calculation

The Gibbs criterion is a useful tool to estimate whether a chemical reaction can take place or not. To start a reaction, the change of Gibbs free energy must satisfy Equation (8) below:

(8)

P_s, P_s^Θ, P_f, P_f^Θ, and ΔG^Θ stand for partial pressure of products, standard partial pressure of products, partial pressure of reactants, standard partial pressure of reactants, and standard Gibbs free energy, respectively [1,2,3,4,5,6,7,8].

To calculate Gibbs free energy, two hypotheses are given as: (1) the air involved in the corrosion is exclusively the H₂O and the O₂; (2) the partial pressure of the H₂O (47,307.1 Pa) and the O₂ (53,992.9 Pa) at the interface of the pure Fe and the Na₂SO₄ are similar to that in the furnace. The calculated results, listed in Table 1, show that the corrosion reactions are favorable on thermodynamic considerations under the experimental conditions. The quantity of H₂SO₄ in the tested conditions is much lower than the theoretically thermodynamic value, and thus the deduced corrosion mechanism is supported by the thermodynamic calculations.

Table 1. Thermodynamic calculation results.

Reactions	Conditions
4Fe + 3O2 + 2H2O + 2Na2SO4 → NaFeO2 + 2H2SO4	PH2SO4 < 19,090.3 Pa
H2SO4 + Fe → FeSO4 + H2	PH2 < 1.02 PH2SO4
6FeSO4 + O2 + 6H2O → 2Fe3O4 + 6H2SO4	PH2SO4 < 42,116.9 Pa
5FeSO4 + O2 + 5H2O → Fe2O3 + Fe3O4 + 5H2SO4	PH2SO4 < 41,040.8 Pa
4Fe + 3O2 + 2Na2SO4 → 4NaFeO2 + 2SO3	PSO3 < 42,491.1 Pa

Table 1. Thermodynamic calculation results.

Reactions	Conditions
4Fe + 3O2 + 2H2O + 2Na2SO4 → NaFeO2 + 2H2SO4	PH2SO4 < 19,090.3 Pa
H2SO4 + Fe → FeSO4 + H2	PH2 < 1.02 PH2SO4
6FeSO4 + O2 + 6H2O → 2Fe3O4 + 6H2SO4	PH2SO4 < 42,116.9 Pa
5FeSO4 + O2 + 5H2O → Fe2O3 + Fe3O4 + 5H2SO4	PH2SO4 < 41,040.8 Pa
4Fe + 3O2 + 2Na2SO4 → 4NaFeO2 + 2SO3	PSO3 < 42,491.1 Pa

4. Experimental Section

4.1. Materials and Experimental Conditions

In this work, pure Fe (99.9%) was employed as the experimental specimen. Before experiments, the sample was cut into coupons with a dimension of 10 mm × 15 mm × 2 mm, ground with silicon-carbide abrasive paper finally to 1000 grit, degreased in acetone and ethanol, and then dried in air. Na₂SO₄ was deposited on the preheated Fe coupon surface by repeatedly brushing and drying with a Na₂SO₄-saturated solution. The mass of the Na₂SO₄ was about 4 mg/cm².

All corrosion experiments were carried out at 500 ± 10 °C. The temperature of the water bath to produce H₂O vapor was fixed at 80 °C (46.8 vol%) and the flux of the O₂ was 200 mL/min.

4.2. Mass Gain Measurements

The corrosion tests were carried out in a thermal balance [1,2,3,4,5,6,7,8]. Water (H₂O) came from an 80 °C water bath. Pure O₂ was passed through the glass bubbler with a flux of 200 mL/min. To prevent condensation of the water vapor in the upper part of the thermal balance, a counter-flow of N₂ was passed through the apparatus at 150 mL/min. After the furnace was heated to the desired temperature and the gas flow was stabilized, the specimen was quickly suspended into the furnace tube, and the test was started. All the measurements were carried out at ambient pressure. There were five parallel samples for each test.

After the tests, the specimens were further examined by XRD and SEM/EDX.

4.3. Electrochemical Experiments

A special three-electrode system was built for the electrochemical measurements in this particular environment (shown in Figure 12) [9]. To decrease the resistance of the solution and get a uniform electric field, the reference electrodes consisted of four platinum wires with a diameter of 0.4 mm, and the counter electrode was a circular strip of platinum foil with a width of about 2 mm. All potential values in this paper were reported versus the platinum reference electrode. The Fe working electrode was a rod with a length of 10 mm and a diameter of 5 mm. The three electrodes were in quartz tubes, which acted as insulators. All the gaps were sealed by high temperature inorganic glue. The three-electrode system after the solid Na₂SO₄ deposition was directly put into the furnace at the desired temperature with the water vapor for electrochemical measurements.

Figure 12. Schematic diagram of three-electrode cell: (A) the top view; (B) the cross-section view.

Figure 12. Schematic diagram of three-electrode cell: (A) the top view; (B) the cross-section view.

The PAR2273 Electrochemical Measurement System manufactured by EG&G was used for all electrochemical measurements, which also has the function to compensate the resistance between reference electrode and working electrode. In the galvanic corrosion measurement, the ratio of anodic area to cathodic area is 1:2. In EIS measurements, the AC perturbation was 0.1 V because of the low conductivity of Na₂SO₄ at 500 °C [21,22] and the frequency was swept from 10 kHz to 10 mHz. The resistance between reference and working electrodes was compensated during measurements according to the design of the electrochemical system and testing work station. The measurements were repeated more than three times.

5. Conclusions

The corrosion rate of the pure Fe is significantly accelerated under a Na₂SO₄ deposit in an atmosphere of H₂O + O₂ at 500 °C. The introduction of H₂O improves the formation of the NaFeO₂ and the H₂SO₄, which accelerates the chemical reactions during the entire corrosion. The occurrence of the electrochemical corrosion reaction promotes the progress of the chemical corrosion reaction. Both of them accelerate the corrosion of the pure Fe. Also, the deduced corrosion reactions were confirmed by thermodynamic calculation.

Acknowledgments

The investigation is supported by the National Natural Science Fund of China under the contract No. 51371181 and National Basic Research Program of China, Ministry of Science and Technology China under the contract No. 2014CB643303.

Author Contributions

The tests were carried out by Yanbing Tang, characterization was performed by Li Liu and Ying Li, the experimental scheme was framed Fuhui Wang. The manuscript was composed by Yanbing Tang and revised by Li Liu and Lei Fan.

Conflicts of Interest

The authors declare no conflict of interest.