Jump to ContentJump to Main Navigation
Show Summary Details
More options …

Open Chemistry

formerly Central European Journal of Chemistry

IMPACT FACTOR 2018: 1.512
5-year IMPACT FACTOR: 1.599

CiteScore 2018: 1.58

SCImago Journal Rank (SJR) 2018: 0.345
Source Normalized Impact per Paper (SNIP) 2018: 0.684

ICV 2017: 165.27

Open Access
See all formats and pricing
More options …
Volume 16, Issue 1


Volume 13 (2015)

Production and Analysis of Recycled Ammonium Perrhenate from CMSX-4 superalloys

J. Gonzalez-Rodriguez
  • Corresponding author
  • School of Chemistry, University of Lincoln, Joseph Banks Laboratories, Green Lane, Lincoln, LN67DL, United Kingdom
  • Email
  • Other articles by this author:
  • De Gruyter OnlineGoogle Scholar
/ Katherine Pepper / M.G. Baron
  • School of Chemistry, University of Lincoln, Joseph Banks Laboratories, Green Lane, Lincoln, LN67DL, United Kingdom
  • Other articles by this author:
  • De Gruyter OnlineGoogle Scholar
/ S.K. Mamo
  • School of Chemistry, University of Lincoln, Joseph Banks Laboratories, Green Lane, Lincoln, LN67DL, United Kingdom
  • Other articles by this author:
  • De Gruyter OnlineGoogle Scholar
/ A.M. Simons
  • School of Chemistry, University of Lincoln, Joseph Banks Laboratories, Green Lane, Lincoln, LN67DL, United Kingdom
  • Other articles by this author:
  • De Gruyter OnlineGoogle Scholar
Published Online: 2018-12-31 | DOI: https://doi.org/10.1515/chem-2018-0136


The process to extract rhenium from a superalloy is an immense technical challenge due the complex chemistry involved. Being one of the rarest elements in the earth’s crust the scarcity and cost of rhenium makes it advantageous to recover the element from scrap superalloy. In this research the separation and monitoring of the different stages of the recycling process to extract rhenium from CMSX-4 superalloys using a distillation process were performed. This novel method combining distillation and use of exchange resins was used to separate rhenium from a complex mixture of metals in the CMSX-4 superalloy. The identification and quantitation of perrhenate and contaminants were performed by atomic absorption spectroscopy (AAS), Fourier transform infrared spectroscopy (FTIR), ion chromatography (IC) and Scanning Electron Microscopy- Energy Dispersive X-Ray (SEM-EDX). Perrhenate ions were extracted with purity close to 93%. The analytical characteristics for a novel infrared method to quickly identify perrhenate anions from CMSX-4 are presented. The main characteristics of the analytical validation were: LoD: 0.5% w/w; LoQ: 1.5% w/w; linear range 1.5-100% w/w; correlation coefficient R2 = 0.9905; precision (%RSD) for 10%w/w = 6.6 and 75%w/w = 4.1, respectively; accuracy (%) for 10% w/w 99.6% and 75% w/w=101.1, respectively.

Keywords: Rhenium; CMSX-4; superalloys; metal recycling; metal separation

1 Introduction

A super alloy, being a unique high temperature and high performance alloy, displays excellent resistance to mechanical and chemical degradation close to their melting points [1]. In addition, super alloys demonstrate increased mechanical strength, creep resistance at high temperatures, good surface stability, and corrosion and oxidation resistance. Furthermore, as they maintain their properties at elevated temperatures (above 540 ̊C), super alloys can be employed in the hottest sections of turbines [2]. As a consequence of technological advances in super alloys, manufacturing costs have increased. Moreover, super alloys require the use of rare and expensive elements, such as rhenium or ruthenium. The alloying elements and heat-treatments also often make superalloys difficult to machine and weld, increasing fabrication costs, part reject rates, and reworks [3].

Rhenium is one of the rarest and most valuable elements in nature, and can only be found distributed on the earth’s surface in very small quantities, on the order of 10-9% [4]. Moreover, it occurs in a scattered form, and methods for its separation – in the form of metal or compounds – are complicated and costly. These factors result in a high price for rhenium and its compounds. Rhenium can be found in copper sulphide ores, but predominantly it can be obtained through molybdenum refinement. After its isolation, rhenium is traded commercially as sodium and ammonium perrhenates. In addition to its use in super alloys, specific properties of rhenium also make it useful for other selective applications, including catalysis and radiology and applications in the nuclear industry.

Rhenium has a range of very desirable mechanical properties that makes it a valuable alloying element. This element has an extremely high density of 21.04 g/cm3, a melting point of 3180°C and a boiling point of 5630°C [5]. Another useful mechanical property is its high ductility, and it does not exhibit a ductile/brittle transition, so it remains ductile up to its melting point. It also presents high strength at elevated temperatures together with a high modulus of elasticity. Rhenium has excellent creep resistance due to its high re-crystallisation temperature of 2800°C, and it withstands vigorous thermal cycling without deterioration.

Being so rare and costly to extract makes it advantageous to recover rhenium from scrap superalloy material. This scrap can take the form of worn component parts or the waste material resulting from the casting process in the production of component parts [3].The process to extract rhenium from a superalloy is a technical challenge due to its complex chemistry, such as the high melting point of the superalloy itself and the high number of oxidation states of other metals present in the mixture. Rhenium, with electron configuration [Xe] 4f14 5d5 6s2, has nine known oxidation states ranging from −1 to +7. The most common rhenium compounds are the oxides and the halides, exhibiting a broad oxidation number spectrum. Once extracted, rhenium is commercially traded in the form of ammonium perrhenate (APR), a white, water soluble salt (NH4ReO4). Rhenium can be obtained from ammonium perrhenate by reducing the salt with hydrogen at high temperatures following the reaction:

2 NH4ReO4 + 7H2 → 2Re + 8H2O + 2NH3

Some studies have been proposed to examine the extraction of rhenium from different matrices. Three major themes emerge repeatedly throughout the literature for the hydrometallurgical extraction of rhenium - solvent extraction, ion exchange and distillation. Zhan-Fang et al. [6] recovered rhenium from an alkaline leach solution of an ore containing rhenium and molybdenum by repeated solvent extraction to obtain rhenium salts with an efficiency of 96.8% [6]. The feed solution in this work came from leaching an ore sample with a composition of molybdenum, 47.4%, and rhenium, 0.07%, the remainder being S, Cu, P, Fe, As, CaO, SiO2 and Sn.

Other methods found in the literature include the extraction of perrhenates using an ion exchange column. Studies outlined by Leszczynska-Sejda et al. [7] suggested two methods for the synthesis of perrhenic acid and its extraction: the sorption of the perrhenate ion on selective anion exchange resins and the sorption of ammonium ion on selective cation exchange resins. The latter was more effective, producing yields of 88%, whilst the former proved ineffective, producing yields that never exceeding 6%. Low levels of contaminants, including NH4+, Na+, K+, Mg+2 and Ca+2, were found in the extract.

Koyama [8] studied the separation of rhenium from technetium by a distillation method due to the similarity in chemical properties of the two elements. Steam distillation was found to be the most effective method for this particular experiment. The samples used in this procedure were pure standards; the purity of the product was not stated within the paper, although they stated that almost 100% of the rhenium was distilled out.

The analysis of rhenium and rhenium salts traditionally has been performed using atomic techniques, such as Atomic Absorption Spectroscopy [9,10]. More recent methods have used inductively coupled plasma mass spectrometry (ICP-MS) to determine rhenium in water [11] and geological materials [12]. Extended X-ray Absorption Fine Structure (EXAFS) has also been used to study the structural properties of rhenium complexes and to interpret extraction mechanisms [13]. Electrochemical analysis of rhenium has also been developed in order to estimate rhenium content in the liqueur from the process of recycling catalysts [4].

The use of spectroscopic techniques for the analysis of the different rhenium complexes using Raman has been also studied [14]. However, these studies are not so abundant for perrhenates (Re (+7)). The most recent study in this sense is attributed to Gassman et al. [15], who presents the capabilities of rhenium as a surrogate material for the safe disposal of technetium in the nuclear industry. Even less information can be found concerning the infrared analysis of perrhenates [14]. Palant et al. [16] developed some work on the infrared analysis of organic complexes using Re (+7) in order to favour its extraction from acidic solutions. Further work has been developed in this area by Cao et al. [17] who used complexes to selectively trap perrhenate and pertechnate before IR analysis.

The importance of recycling and recovery of metals from used materials is growing. Mining costs and the difficulty of access to some ores makes recycling a more economically viable alternative for many metals. According to Hunt et al. [18], at the present rate of extraction, the reserves of rhenium will be depleted in 50-100 years. This implies that a policy of elemental sustainability and critical element recovery needs to be implemented if we want to maintain the current applications and, most important, to guarantee use for future generations. Rhenium recycling remains a challenging problem, and no definite answer has been found from an industrial point of view. To date, the most effective recycling method for rhenium in a real case is when this element is combined with platinum and recovered from automobile catalytic converters. In this case, the chemical nature of platinum and the fact this is a binary mixture makes it easy to extract, leaving rhenium behind.

In this work, the extraction and purification of rhenium from a complex nickel-based superalloy known as CMSX-4 was investigated. For this procedure, we utilised a fractional distillation process combined with ion exchange and precipitation to produce high purity ammonium perrhenate (APR). A novel infrared method was also implemented for the fast determination of the ammonium perrhenate content in the recycled powder.

2 Material and Methods

2.1 Chemicals and methods

2.1.1 Dissolution and distillation method

CMSX-4 is a second generation nickel-based superalloy with a typical composition of: chromium (6.5%), cobalt (9.6%), tungsten (6.4%), rhenium (3%), molybdenum (0.6%), aluminium (5.6%), titanium (1%), tantalum (6.5%), hafnium (0.1%) and nickel (60.7%). In order to extract the different metals from the superalloy aqua regia, a mixture of concentrated hydrochloric acid (36%, 11.65 M) and concentrated nitric acid (70%, 15.8 M) in a 3:1 ratio, was used. Both acids were purchased from Merck (Darmstadt, Germany). One hundred grams of CMSX-4 were mixed with one litre of the aqua regia solution in a polypropylene container and placed in the fume cupboard using a venturi scrubber to prevent any release of gases to the environment for 5 hours. Any solids produced at this stage were removed and the supernatant transferred to another container. The next stage consisted of the sequential addition of NaOH (Merck) pellets to the metal solution. This was performed under constant stirring and pH monitoring until the solution reached pH 13. The various solids obtained during the sequential precipitation after sodium hydroxide addition were removed. The supernatant was then subjected to both a clean-up and preconcentration process using a Dowex Marathon A: Type 1 Strong Base Anion Exchange Resin (Dow Chemical Co) to trap the anions present in the solution. Four hundred and eighty millilitres of this solution were added to 6 grams of resin, and the mixture was stirred on a magnetic stirrer for 30 minutes. The resin was filtered from the solution and placed into a one-litre beaker with 250 mL of 21.6% HCl, and the slurry was stirred for 45 minutes. This procedure ensured the extraction of the anions absorbed on the resin into the solution. The final step prior to distillation was filtering off the resin to leave a solution containing the target analyte, perrhenic acid, and other residual anions.

Three hundred and fifty millilitres (350 mL) of the enriched perrhenic acid solution were placed into a distillation bulb with 50 mL of concentrated sulphuric acid using a distillation setup as shown in figure 1. The temperature was recorded until the system reached 185oC, when the source heating was turned off and the system allowed to fully cool down. The collecting bulb containing this first fraction was then removed and replaced with a new bulb. An additional 350 mL of deionised water were added to the original main distillation bulb, and the mixture was carefully stirred. Heating was reinitiated and temperature recorded to repeat five cycles in total. At this point the distillation was complete. This process of sequential re-distillations serves the purpose of cleaning up the sample and obtaining a high purity perrhenic acid solution.

Distillation set up for the separation of perrhenic acid in solution.
Figure 1

Distillation set up for the separation of perrhenic acid in solution.

In order to obtain the final product, ammonium perrhenate (APR), 40 mL of concentrated (25%) ammonia solution (Merck) was added to the perrhenic acid solution obtained from the distillation process. The mixture was then placed onto a heating mantle and the solvent evaporated off until a small amount of white solid was visible in the solution and a precipitate obtained. At this stage the heating was discontinued. After this step, the samples were left to cool down and then placed into a refrigerator at 4oC for 12 hours to favour further precipitation. The precipitated salt was separated from the supernatant by vacuum filtration and left to dry in a desiccator.

Flow diagram for the production of Ammonium Perrhenate from CMSX-4 superalloy.
Scheme 1

Flow diagram for the production of Ammonium Perrhenate from CMSX-4 superalloy.

Scheme 1 illustrates the stages in the production of APR.

2.2 Instruments

Flame atomic absorbance analysis of the powder samples was performed on a Thermo Unicam 969 (Waltham, MA, USA). The spectrometer used a 37 mm single element rhenium hollow cathode lamp using a wavelength of 346.1 nm, lamp current of 75 mA and a band pass of 0.5 nm. The flame was generated using nitrous oxide and acetylene with a flow of 3.9 g/L and a flame stabilisation of 4. Calibration was performed using a 1000 ppm rhenium standard which was diluted to make standards of 5 mg/L, 10 mg/L, 20 mg/L, 30 mg/L, and 50 mg/L. All samples and standards were made up using 15 MΩ deionised water.

For infrared analysis, a Perkin Elmer Spectrum 100 FT-IR Spectrometer (Waltham, MA, USA) fitted with a Specac- Standard Golden Gate ATR attachment was used. Ten milligrams of sample were placed on the ATR for analysis, which was performed at mid infra-red: 450-4000 cm-1 using 16 scans and a resolution of 4 cm-1.

A Dionex ICS 1100 Ion Chromatograph (Waltham, MA, US) attached to an AS-DV auto sampler was used to analyse the samples for chlorides, nitrates and sulphates. Specification requirements were a 150mm column, a flow rate of 1 ml/min, an injection volume of 10μl, and sample run times of 18 minutes for standards and 30 minutes for unknown samples. The eluent was 8.0mM sodium carbonate and the regenerant 2N sulphuric acid.

An FEI Inspect SEM attached to an INCAx-act EDX detector from Oxford Instruments (Abingdon, Oxfordshire, UK) using INCA Software was used for the analysis of metals in the powder.

Equilibrium analysis of the different metals in solution was performed with MEDUSA (Make Equilibrium Diagrams Using Sophisticated Algorithms software) (Ignasi Puig Domenec, Royal Institute of Technology, Stockholm, Sweden).

Ethical approval: The conducted research is not related to either human or animal use.

3 Results and Discussion

The dissolution process of CMSX-4 is a complex process, and thermodynamics and kinetic properties of the ten different metals that constitute this alloy need to be considered. First, the selection of the dissolution agent is critical. Aqua regia will favour the highest oxidation states and will take the initial pH values below zero. Thermodynamic considerations for the process, and how they may affect the equilibrium for the different metals at the different pH values, will determine the species present in solution. Table 1 shows a summary of these species at different pH values using the model produced for each metal by MEDUSA software. Interactions between metals are not accounted for in the models.

Table 1

Different speciation for the different metals depending on pH, where the shading indicates the presence of a precipitate.

Thermodynamic modelling shows that tungsten is oxidised to WO3, which is insoluble in a pH range from -1 to 2. A similar situation was observed for tantalum, which presented a solid phase of Ta2O5 at the pH used during the dissolution process. These insoluble complexes, coupled with incomplete leaching due to slow kinetics, explains why CMSX-4 was not fully dissolved following 5 hours of leaching in aqua regia. A gradual increase of the pH of the solution induced the precipitation of other metal species at different pH values (see Table 1) in such a way that, according to the thermodynamic models, at pH 13 only chromium and rhenium should remain in solution, provided other metals are filtered away as they form. ICP-OES (outsourced) analysis of a similar solution generated from aqua regia

leaching of CMSX-4 followed by raising the pH to 8 shows that, of the metals in the super alloy, only rhenium is present in a significant concentration (667 mg/L). All other metals (Ti, Ta, Mo, Cr, Ni, Al, Co) were present at less than 2 mg/L in solution, which suggests that the thermodynamic modelling is incorrect with respect to chromium. This error could be due to the formation of more complex species that are not accounted for in the thermodynamic database used. This selective precipitation was the first clean-up process and eliminated most of the metals that could contaminate or interfere with the extraction of rhenium. A relatively clean solution was obtained, and the next stage of the process could then be started.

Ion exchange was used to further purify the liqueur. An ion exchange resin was used to trap the perrhenate ions produced in the dissolution process. It also eliminated any neutral and cationic contaminants that might have been left in solution, including significant amounts of sodium present from the use of sodium hydroxide during neutralisation. At this stage only rhenium was adsorbed and retained on the resin. These anions were later eluted with hydrochloric acid to produce a purer solution that was presented for distillation.

A five-stage partial distillation process was followed. As seen in the results of this process (Figure 2), the first stage of the distillation presented a plateau around 106oC, which is consistent with the distillation of hydrochloric acid and with the acidic fumes that were observed during the distillation process at this temperature. This plateau only appeared in the first two first stages and was not observed during the remaining stages. The distillation of HCl explains the consistent lack of chlorides in the final product, as could be seen when the product was analysed by SEM-EDX (Figure 3). The lack of chlorides in most of the final fractions was also confirmed by ion chromatography analysis (data not shown).

Distillation model for the purification process of APR.
Figure 2

Distillation model for the purification process of APR.

Another feature that can be observed in the distillation curves is a shoulder around 121oC, which is consistent with the distillation of nitric acid which was carried over from the leach solution during ion exchange. Distillation of HNO3 also explained the absence of nitrate in most of the purified products. Further analyses demonstrated that little to none of the acids used during the initial dissolution with aqua regia or elution of the ion exchange resin remained in the distilled solutions beyond the third fraction.

The next characteristic feature observed in the distillation curves is a plateau around temperatures just above 150o C. This plateau is consistent with the distillation of perrhenic acid. Distillation of the desired acid is also supported by the analysis of fractions 3 and 4, as these showed the highest concentrations of this acid. It is worth noting that higher concentrations were directly related to the length of this plateau (at constant temperature for longer times). The longer the plateau, the higher the concentration of perrhenic acid obtained.

Sulphuric acid, which was added to acidify the solution before distillation, boils at 337oC, a temperature never reached during the distillation process. Nonetheless, a considerable amount of sulphuric acid can be dragged by water molecules when they evaporate, and this phenomenon can explain why sulphates were the main contaminant ions in the purified powder, as confirmed by ion chromatography.

SEM-EDX analysis of the purest distillation fraction.
Figure 3

SEM-EDX analysis of the purest distillation fraction.

The final stage of the separation process, precipitation of ammonium perrhenate (APR), was performed by adding ammonia solution to the purest distillate (enriched perrhenic acid solution in fraction 4). The precipitation powder was analysed by SEM-EDX (Figure 2), AAS and ion chromatography, and the results showed no other metals or contamination other than sulphates (data not shown).

The various options for the analysis of the powder produced at the end of the process were also a subject of this study. However, little information or research exists on the monitoring of rhenium in the extraction and recycling from super alloys using molecular spectroscopic techniques, such as FTIR, in order to assess the purity of the products obtained in the process. Moreover, currently published research lacks discussion of contaminants from the refining process. Additionally, the non-destructive nature of FTIR, fast analysis time, and little or no requirement for sample preparation are obvious advantages of using a molecular spectroscopic method. Furthermore, this technique was also able to provide analysis of rhenium compounds at molecular level.

Hence, FTIR proved to be a convenient and effective method to allow for molecular identification, and it was a particularly powerful method alongside Atomic Absorption Spectroscopy (AAS), which provided the elemental analysis. AAS determined rhenium concentrations (mg/L) in the different unknown powders, whereas FTIR allowed for distinct chemical structure identification. In combination, these data, in comparison to known standards, permitted complete identification of components of a powder. This allowed for direct APR identification along with the ability to identify the various contaminants present in the sample, which AAS analysis alone could not provide.

The IR analysis of an ammonium perrhenate standard against a potassium perrhenate standard allowed for a greater understanding of the signal obtained from NH4ReO4. The NH4ReO4 standard exhibited three peaks in the medium IR spectrum, whereas the KReO4 standard only displayed one peak in the same IR range. The common peak obtained for the two standards corresponded to ReO4 ion (Figure 4). As potassium ion is IR transparent over the entire range of wavelengths, a peak for this ion would not be expected. Subsequently it can be deduced that the triple peak obtained in the wavelength range from 2783 to 3304cm-1 and that at 1448cm-1 are associated with the NH4+ ion [19] and the overlap peaks for both compounds at 913 cm-1 is related to the perrhenate (ReO4-) ion. The band obtained is very close to the band observed by Cao et al 17 at 910 cm-1 for ReO4 in the [(CuCl)3L](PF6) (ReO4)2⋅3H2O complex.

Ammonium perrhenate IR spectrum compared to potassium perrhenate spectra.
Figure 4

Ammonium perrhenate IR spectrum compared to potassium perrhenate spectra.

In FTIR, the peak intensity can be directly related to the concentration of the chemical species of interest, as IR spectroscopy follows the Beer-Lambert Law. For this, reason a range of APR standards at different concentrations were prepared to allow for the determination of peak intensities, and hence, when applied to the powders

produced, an estimation of APR concentration could be calculated. The same process was followed to evaluate the presence of sulphates in the powders, as this is the main contaminant likely to be present, as demonstrated by both SEM-EDX and ion chromatography analyses. A summary of the analytical characteristics of the method were produced and can be found in Table 2.

Table 2

Analytical characteristics of the Infrared determination of APR and sulphates in the recycled samples.

The determination of perrhenate allows for enhanced analysis as compared to sulphate complexes in the recycled matrix. The limits of detection and quantitation are also better for perrhenates than for sulphates. The linearity range is similar, and the method is suitable for the determination of main impurities found in the powder samples. If sulphates are present in very low concentrations, quantification is difficult. The precision and accuracy at higher concentrations for both ions are within acceptable limits. At lower concentrations the precision and accuracy for sulphates are not as good as for perrhenates but still within acceptable limits for a screening method. This was to be expected given that FTIR is not a particularly sensitive technique. Practically, these considerations are relatively unimportant to industrial applications, as the concentrations likely to be found for each of these compounds are much higher than those calculated for the LoD and LoQ. From the samples analysed after the recycling process, the amounts of sulphate and perrhenates found were always able to be assessed using spectroscopy, and results matched those obtained for atomic absorption or chromatography.

Figure 5 shows the correlation found between the responses obtained for AA analyses and FTIR for a set of 16 APR samples produced from the distillation process. It can be seen that, in general terms, both techniques can be considered statistically comparable as there is a distinct correlation between the two data sets. The experimental results obtained present a slope of 1.033 and an intercept

Correlation between FTIR and AA purity results.
Figure 5

Correlation between FTIR and AA purity results.

Two powder samples obtained from the purification process. Blue line: ReO4– (8.5%) and SO4– (71.3%) and red line: ReO4– (92.4%) and SO4– (6.9%).
Figure 6

Two powder samples obtained from the purification process. Blue line: ReO4 (8.5%) and SO4 (71.3%) and red line: ReO4 (92.4%) and SO4 (6.9%).

of -0.342 with a correlation coefficient of R2=0.991. As the slope is close to 1 and the intercept is close enough to zero we can establish that there is a close relationship between the values for AAS and FTIR as there is also a good correlation.

In order to identify and determine APR in complex mixtures, the determination of potential contaminants was performed in the recycled powder to assess the robustness of the method. A range of samples obtained following the recycling procedure were analysed using ion chromatography for the presence of nitrates, chlorides and sulphates, as these were the typical contaminants likely to be found in the recycled powders, and the purity of rhenium (as %Re) was calculated using AA. Figure 6 shows an example results from two very different samples in which the concentrations of rhenium and sulphate were 18.5% and 71.3%, respectively, for the first sample and 92.4% and 6.9% for the second sample. It was also noticed that, in general, an increasing concentration of sulphates and contaminants had the ability to shift the perrhenate peak towards longer wavenumbers. In this way, a concentration of 6.9% in sulphate concentration would allow the perrhenate peak to be measured at 871 cm-1, while a highly contaminated sample with a concentration of sulphates of 71.3% would shift the perrhenate peak to 915 cm-1, showing it as a shoulder on the slope of the sulphate peak (indicated by the arrow in Figure 6). These cases were also considered and included in the estimation of the experimental error of the method. The shifting of the perrhenate peak did not particularly affect the ability of this method to identify the different species or to calculate accurate concentrations. In some particular cases, where a very small amount of nitrates were found in the powders, the peak appeared at 1400 cm-1, which is far from those of sulphates or perrhenates. Given this result, nitrates are not considered an interference for perrhenate or sulphate quantification. Chlorides are transparent in infrared spectroscopy and also not a problem for the determination of rhenium.

Table 3 displays a typical example of data obtained from the distillation process. Ion chromatography confirmed that no nitrates were found and only small amounts of chlorides were present in these two powder samples. For this case, fractions 3 and 4 were found to have sulphate contaminations of 6.92% and 6.87%, respectively. Accordingly, it can be argued that FTIR can be used as a technique to provide information on the rhenium content but also to aid in the identification of contaminants within the powders as the peaks for sulphates and rhenium were identified and concentrations accurately calculated.

Table 3

Ion chromatography results for an example distillation result for fractions 3 and 4.

4 Conclusions

The separation and monitoring of the different stages of a recycling process to extract rhenium from a CMSX-4 superalloy and produce ammonium perrhenate (APR) were performed. The identification and quantitation of this anion and main contaminants present from the extraction process were performed by Atomic Absorption Spectroscopy (AAS), Fourier transform infra-red spectroscopy (FTIR), Scanning Electron Microsocopy - Energy Dispersive X-Ray (SEM-EDX) and ion chromatography (IC). AAS allowed for elemental identification and quantitation of the rhenium present in the sample, whereas FTIR provided the crucial aspect of molecular identification to determine whether APR was effectively produced. Using ion chromatography, SEM-EDX and AAS, some of the main contaminants present in the final product were also identified and quantitated. FTIR also succeeded in monitoring the most important

contaminants both qualitatively and quantitatively. These were identified to be nitrates, chlorides and sulphates coming from the different acids used in the separation process. No other metals but rhenium were found in the APR samples obtained from the recycling process. Samples obtained from the CMSX-4 superalloy were then successfully recycled and analysed, opening an interesting door for the re-utilisation of this scarce metal.

To the best of our knowledge, no research is available in the literature on the analysis of APR by FTIR spectroscopy with the aim of identification and quantitation of this anion from CMSX-4 superalloy extracts. From an analytical point of view the characteristics for an infrared method to identify perrhenate anions extracted from CMSX-4 have been presented and a comparison with the atomic absorption method used, as a reference standard demonstrated that there are no statistically significant differences between the two methods. Subsequently, it has been established that although atomic absorption spectroscopy continues to provide useful elemental information, FTIR spectroscopy can provide considerably fast quantitative and qualitative analysis in the recycling process of the superalloy CMSX-4.


The researchers want to thank Praxair Surface Technologies Ltd. for the economic support given to Mrs Pepper during the realisation of this research.


  • [1]

    Reed R.C., The Superalloys: Fundamentals and Applications, Cambridge University Press, 2006. Google Scholar

  • [2]

    Sims C.T., Stoloff N.S. and Hagel W.C., Superalloys II, John Wiley & Sons, 1987. Google Scholar

  • [3]

    Donachie M.J. and Donachie S.J, Superalloys; A Technical Guide, 2nd ed., ASM International, 2002. Google Scholar

  • [4]

    Gopalakrishnan, K. and Koshy, V.J., Differential Pulse Voltammetric Estimation of Rhenium in Catalysts and Process Solutions, Electroanalysis 1998, 10, 54-57. Google Scholar

  • [5]

    Cotton, F.A. and Wilkinson, G., 5th ed., Advanced Inorganic Chemistry, John Wiley & Sons, 1988. Google Scholar

  • [6]

    Zhan-Fang, C., Hong, Z., Zhao-Hui, Q., Solvent Extraction of Rhenium from Molybdenum in Alkaline Solution, Hydrometallurgy, 2009, 97, 153-157. CrossrefWeb of ScienceGoogle Scholar

  • [7]

    Leszczynska-Sejda, K., Benke, G., Chmielarz, A., Krompiec, S., Michalik, S. and Krompiec, M., Synthesis of Perrhenic Acid using Ion Exchange Method, Hydrometallurgy, 2007, 89, 289-296. Web of ScienceCrossrefGoogle Scholar

  • [8]

    Koyama M., Chemical Studies on Radioactive Indicators: XXIV: Separation of Rhenium from Technetium by the Distillation Method, Bull. Chem. Soc. Jpn., 1961, 34, 1766-1769. CrossrefGoogle Scholar

  • [9]

    Tomkins D.F., Frank C.W., Appl. Spectrosc., 1971, 25(5), 539-541. CrossrefGoogle Scholar

  • [10]

    Yudelevich I.G., Zelentsova L.V., Beisel N.F., Chanysheva T.A., Vechernish L., Anal. Chim. Acta, 1979, 108, 45-52. CrossrefGoogle Scholar

  • [11]

    Uchida S., Tagami K., Saito M., J. Radioanal. Nucl. Chem., 2003, 255(2), 329-333. CrossrefGoogle Scholar

  • [12]

    Meisel . T., Moser J., Chem. Geol., 2004, 208(1-4), 319-338. CrossrefGoogle Scholar

  • [13]

    Suzuki S., Yaita T., Okamoto Y., Shiwaku H., Motohashi H., Phys Scr Vol T, 2005, T115, 306-307. Google Scholar

  • [14]

    Petrov K. I., Pervykh V. G., Varfolomeev M. B., Plyushchev V. E., J. Appl. Spectrosc., 1968, 8(4), 401-404. CrossrefGoogle Scholar

  • [15]

    Gassman P. L., McCloy J. S., Soderquist C.Z., Schweiger M. J., J. Raman Spectrosc., 2014, 45, 139-147. CrossrefGoogle Scholar

  • [16]

    Palant A.A. , Petrova V.A., Yatsenko N.A., Russ. J. Inorg. Chem., 1998, 43(2), 283-286. Google Scholar

  • [17]

    Cao R., McCarthy B. D., Lippard S. J., Inorg. Chem. 2011, 50(19), 9499–9507. CrossrefPubMedGoogle Scholar

  • [18]

    Hunt A.J., Matharu A. S., King A. H., Clark J. H., Green Chem., 2015, 17, 1949–1950. CrossrefGoogle Scholar

  • [19]

    NIST Standard Reference Data, 2011, Available from: http://webbook.nist.gov/cgi/cbook.cgi?ID=B6000448&Mask=80#IR-Spec [last accessed 13/11/15]. 

About the article

Received: 2018-06-06

Accepted: 2018-10-09

Published Online: 2018-12-31

Conflict of interest Authors declare no conflict of interest.

Citation Information: Open Chemistry, Volume 16, Issue 1, Pages 1298–1306, ISSN (Online) 2391-5420, DOI: https://doi.org/10.1515/chem-2018-0136.

Export Citation

© 2018 J. Gonzalez-Rodriguez et al., published by De Gruyter. This work is licensed under the Creative Commons Attribution-NonCommercial-NoDerivatives 4.0 License. BY-NC-ND 4.0

Comments (0)

Please log in or register to comment.
Log in