Cryo-Mechanical Treatment and Hydrometallurgical Process for Recycling Li-MnO 2 Primary Batteries with the Direct Production of LiMnPO 4 Nanoparticles

: In this work, an innovative hydrometallurgical recycling route for the recovery of all the materials composing Li-MnO 2 primary batteries was proposed. End-of-life batteries were mechanically treated in an innovative pilot plant where a cryogenic crushing was performed. The mechanical treatment allowed for the release of the electrodic powder contained in the batteries with the simultaneous recovery of 44 kg of steel and 18 kg of plastics from 100 kg of batteries. Electrodic powder was employed as the raw material for the synthesis of LiMnPO 4 nanoparticles. To obtain the synthesis precursors, selective sequential leaching of Li and Mn was performed. Li was extracted via water washing the electrodic powder and Li 2 CO 3 and a purity of 99% was recovered. The black mass containing Mn oxides was leached using phosphoric acid, which gave a Mn-bearing precursor solution that was directly used for the hydrothermal synthesis of LiMnPO 4 nanoparticles. A preliminary materials balance of the process was presented, indicating that the proposed process should be an easy hydrometallurgical route for the recycling of primary lithium batteries. In addition, the simultaneous production of high-value-added products that could be reintroduced into the battery manufacturing chain could ensure the economic feasibility of the process.


Introduction
The collection and recovery of batteries in Europe are regulated by the Directive 2006/66/EC, which prohibits the disposal in landfills or incineration of waste batteries and accumulators. The targets set by the legislation are to collect 65% and recover 50% by weight of the batteries [1].
Primary batteries represent about 75% of the total batteries and accumulators placed on the EU market in 2018. Among this kind of battery, alkaline represents 61%, zinc carbon represents 10%, lithium represents 3%, and silver oxide represents 1%. The residual 25% of the total batteries placed on the EU market is composed of secondary batteries (Li-ion: 16%, Ni-MH: 6%) [2]. Li-MnO 2 type, which represents 3% of primary batteries, still presents many critical issues regarding recycling. The presence of highly reactive metallic lithium and organic solvents, which compose the electrolytic solution, entail safety risks during the recycling of these batteries. Li primary batteries are currently treated along with Li-ion batteries in a few big pyrometallurgical plants in Northern EU countries [3,4]. Nevertheless, pyrometallurgical processes do not allow for the recovery of non-metals, such as graphite and carbon, and Li and Mn end up in the slag, which requires additional steps for their recovery [5]. Furthermore, this kind of processing has negative environmental impacts due to the high energy

Lithium and Manganese Extraction and Recovery
The electrodic powder was employed as a raw material for the synthesis of LiMnPO4 nanoparticles. The electrodic powder was neutralized in a mechanically stirred reactor using water at room temperature and with a solid-to-liquid ratio equal to 1:5. The operation was performed to extract the soluble lithium coming from the metallic lithium anode and the electrolyte. After the filtration, the liquid stream was recycled for five subsequent washing operations of the electrodic powder samples. The resulting solution was employed for the precipitation of Li2CO3 at 95 °C; then, Na2CO3 was added. After two hours, the obtained suspension was filtered and oven-dried overnight at 105 °C.
The extraction of manganese from the electrodic powder was attained by leaching for 3 h under stirring at 85 °C with phosphoric acid at concentrations of 1.5 and 3.0 M. Hydrogen peroxide (35% v/v) was used as the reducing agent. A manganese-rich solution was recovered after the leachate filtration and used as the precursor solution in the LMP synthesis.

Synthesis of LiMnPO4
The synthesis of LiMnPO4 (LMP) was adapted from the method of Ji et al. [18]. The manganeserich solution obtained after the electrodic powder leaching was used as a starting solution for the synthesis procedure. The lithium concentration was adjusted by adding the recovered Li2CO3 that was previously dissolved in a sulfuric acid solution. The amounts of acid, lithium carbonate, and leaching solution used were calculated to produce a final concentration of Mn 2+ equal to 0.1 M in a final volume of 50 mL. Keeping the system under constant stirring, commercial LiOH was added until a pH of 11-12 was reached. The yellowish suspension obtained was transferred to a Teflon vessel and microwave heated (Milestone ETHOS 900 -Milestone srl, Sorisole -Italy) for 30 min at a temperature of 180 °C. LMP was obtained after filtration and washing with water, followed by ethanol. The recovered LMP was compared with synthetic LMP produced by applying the abovedescribed method with commercial-grade synthetic reagents.

Lithium and Manganese Extraction and Recovery
The electrodic powder was employed as a raw material for the synthesis of LiMnPO 4 nanoparticles. The electrodic powder was neutralized in a mechanically stirred reactor using water at room temperature and with a solid-to-liquid ratio equal to 1:5. The operation was performed to extract the soluble lithium coming from the metallic lithium anode and the electrolyte. After the filtration, the liquid stream was recycled for five subsequent washing operations of the electrodic powder samples. The resulting solution was employed for the precipitation of Li 2 CO 3 at 95 • C; then, Na 2 CO 3 was added. After two hours, the obtained suspension was filtered and oven-dried overnight at 105 • C.
The extraction of manganese from the electrodic powder was attained by leaching for 3 h under stirring at 85 • C with phosphoric acid at concentrations of 1.5 and 3.0 M. Hydrogen peroxide (35% v/v) was used as the reducing agent. A manganese-rich solution was recovered after the leachate filtration and used as the precursor solution in the LMP synthesis.

Synthesis of LiMnPO 4
The synthesis of LiMnPO 4 (LMP) was adapted from the method of Ji et al. [18]. The manganese-rich solution obtained after the electrodic powder leaching was used as a starting solution for the synthesis procedure. The lithium concentration was adjusted by adding the recovered Li 2 CO 3 that was previously dissolved in a sulfuric acid solution. The amounts of acid, lithium carbonate, and leaching solution used were calculated to produce a final concentration of Mn 2+ equal to 0.1 M in a final volume of 50 mL. Keeping the system under constant stirring, commercial LiOH was added until a pH of 11-12 was reached. The yellowish suspension obtained was transferred to a Teflon vessel and microwave heated (Milestone ETHOS 900 -Milestone srl, Sorisole -Italy) for 30 min at a temperature of 180 • C. LMP was obtained after filtration and washing with water, followed by ethanol. The recovered LMP was compared with synthetic LMP produced by applying the above-described method with commercial-grade synthetic reagents.

Characterizations
The metals content in all the liquid streams emerging from the different process operations were adequately diluted and analyzed using high-resolution continuum source atomic absorption spectroscopy (AAS, contrAA 300-Analytik Jena AG, Jena, Germany). The metals contained in the solid sample were extracted via microwave-assisted leaching (Milestone ETHOS 900) using 10 mL of aqua regia and 0.5 g of the solid sample. The resulting solution was adequately diluted and analyzed using AAS.
To characterize the morphology of the recovered Li 2 CO 3 and LMP, field emission scanning electron microscopy (SEM, Zeiss Auriga-Carl Zeiss, Oberkochen, Germany) was employed. The chemical composition was determined using energy-dispersive X-ray spectroscopy (EDX, Bruker QUANTAX 123 eV-Bruker Corporation, Billerica, Massachusetts). Powder X-ray diffraction (XRD, Rigaku, D-Max Ultima-Rigaku Corporation, Tokyo, Japan) employing Cu Kα radiation was used to identify the crystalline phase of the produced samples.

Recovery of Lithium and Production of the Mn 2+ -PO 4 3− Precursor Solution
The sieving of the crushed batteries produced about a 20% fine fraction and an 80% coarse fraction. The fine fraction, which was mostly composed of electrodic powder (Figure 2A), contained 38.5 ± 0.7 and 420 ± 10 mg g −1 of Li and Mn, respectively. The coarse fraction was mainly composed of the steel and plastic and contained 1 ± 1 and 7 ± 2 mg g −1 of Li and Mn, respectively ( Figure 2B). The steel content of the coarse fraction was about 45% by mass and could be directly recovered. The plastic fraction on the coarse fraction was about 18%. The electrodic powder was washed in water to extract the lithium coming from the residual metallic Li anode, the Li oxidized species formed during the crushing (LiOH, Li 2 O), and from the electrolyte [19].

Characterizations
The metals content in all the liquid streams emerging from the different process operations were adequately diluted and analyzed using high-resolution continuum source atomic absorption spectroscopy (AAS, contrAA 300-Analytik Jena AG, Jena, Germany). The metals contained in the solid sample were extracted via microwave-assisted leaching (Milestone ETHOS 900) using 10 mL of aqua regia and 0.5 g of the solid sample. The resulting solution was adequately diluted and analyzed using AAS.
To characterize the morphology of the recovered Li2CO3 and LMP, field emission scanning electron microscopy (SEM, Zeiss Auriga -Carl Zeiss, Oberkochen, Germany) was employed. The chemical composition was determined using energy-dispersive X-ray spectroscopy (EDX, Bruker QUANTAX 123 eV -Bruker Corporation, Billerica, Massachusetts). Powder X-ray diffraction (XRD, Rigaku, D-Max Ultima -Rigaku Corporation, Tokyo, Japan) employing Cu Kα radiation was used to identify the crystalline phase of the produced samples.

Recovery of Lithium and Production of the Mn 2+ -PO4 3− Precursor Solution
The sieving of the crushed batteries produced about a 20% fine fraction and an 80% coarse fraction. The fine fraction, which was mostly composed of electrodic powder (Figure 2A), contained 38.5 ± 0.7 and 420 ± 10 mg g −1 of Li and Mn, respectively. The coarse fraction was mainly composed of the steel and plastic and contained 1 ± 1 and 7 ± 2 mg g −1 of Li and Mn, respectively ( Figure 2B). The steel content of the coarse fraction was about 45% by mass and could be directly recovered. The plastic fraction on the coarse fraction was about 18%. The electrodic powder was washed in water to extract the lithium coming from the residual metallic Li anode, the Li oxidized species formed during the crushing (LiOH, Li2O), and from the electrolyte [19]. About half of the total Li contained in the electrodic powder was extracted. This less than quantitative extraction could be attributed to the presence of insoluble LiMnO2 produced as the battery discharged (Li + MnO 2  MnOOLi) and, in a minor part, to the formation of organic lithium species generated by the lithium reaction with electrolyte solutions while the batteries discharged [20]. The recovery of lithium was attained through its precipitation as Li2CO3. To obtain a high Li + concentration and reduce the energy needed for concentrating via water evaporation, the washing solution was recycled to neutralize the fresh electrodic powder.
The effect of the number of washing cycles on the lithium extraction was evaluated and the results are reported in Table S1 of the supporting information file. After four washing cycles with the same solution, the lithium reached a maximum concentration of about 4 g L −1 . The recycling of the lithium solution beyond the fourth time resulted in no additional lithium extraction. The liquid phase obtained after the four washing cycles was used for the lithium precipitation with sodium carbonate. The solubility gap between Li2CO3 and Na2CO3 at a temperature close to the boiling point of the system allowed for the precipitation of high-purity Li2CO3. Crystalline Li2CO3 formation was confirmed, both from the SEM analysis of the solid ( Figure 3A) and the XRD analysis of the produced solid. The experimental XRD spectrum matched the Li2CO3 peaks when compared with a reference spectra ( Figure 2B). The impurities in the obtained Li2CO3 were estimated after its dissolution and About half of the total Li contained in the electrodic powder was extracted. This less than quantitative extraction could be attributed to the presence of insoluble LiMnO 2 produced as the battery discharged ( Li + MnO 2 → MnOOLi ) and, in a minor part, to the formation of organic lithium species generated by the lithium reaction with electrolyte solutions while the batteries discharged [20]. The recovery of lithium was attained through its precipitation as Li 2 CO 3 . To obtain a high Li + concentration and reduce the energy needed for concentrating via water evaporation, the washing solution was recycled to neutralize the fresh electrodic powder.
The effect of the number of washing cycles on the lithium extraction was evaluated and the results are reported in Table S1 of the supporting information file. After four washing cycles with the same solution, the lithium reached a maximum concentration of about 4 g L −1 . The recycling of the lithium solution beyond the fourth time resulted in no additional lithium extraction. The liquid phase obtained after the four washing cycles was used for the lithium precipitation with sodium carbonate. The solubility gap between Li 2 CO 3 and Na 2 CO 3 at a temperature close to the boiling point of the system allowed for the precipitation of high-purity Li 2 CO 3 . Crystalline Li 2 CO 3 formation was confirmed, both from the SEM analysis of the solid ( Figure 3A) and the XRD analysis of the produced solid. The Energies 2020, 13, 4004 5 of 11 experimental XRD spectrum matched the Li 2 CO 3 peaks when compared with a reference spectra ( Figure 2B). The impurities in the obtained Li 2 CO 3 were estimated after its dissolution and subsequent AAS analysis of the resulting solution ( Figure 3C). Mn and Fe contents lower than 0.1% were found. Based on these data, the estimated purity of the product was higher than 99%, while about 95% of the lithium contained in the washing solution was recovered.
Energies 2020, 13, x FOR PEER REVIEW 5 of 11 subsequent AAS analysis of the resulting solution ( Figure 3C). Mn and Fe contents lower than 0.1% were found. Based on these data, the estimated purity of the product was higher than 99%, while about 95% of the lithium contained in the washing solution was recovered. To obtain the Mn 2+ and PO4 3− precursors for the LMP synthesis, the extraction of manganese and residual lithium was carried out by leaching the already water-leached electrodic powder with phosphoric acid. Due to the Mn 4+ insolubility, a reducing agent to form Mn 2+ and/or Mn 3+ was needed. For this purpose, hydrogen peroxide was evaluated as a reducing agent by using two different concentrations of H3PO4. The H3PO4 concentrations were chosen to respect the stoichiometry of the following reaction: Considering that the dissociation of H3PO4 was dominated by a single dissociation, two acidic solutions were employed. The first solution contained the stoichiometric amount of H + (1.5 M) to react with Mn, while the second solution contained a 100% excess of H + (3 M). Figure 4 shows the effects of the H3PO4 concentration and reducing agent on the Mn and Li extraction. Using 3.0 M phosphoric acid and 20% (v/v) hydrogen peroxide, the maximum yield of Mn extraction was about 75%. It is well known that Mn compounds, such as MnO2, as well as activated carbon, can catalyze hydrogen peroxide decomposition to produce water and oxygen (Equations (2,3)) [21,22].

Li (mg g -1 )
Mn (mg g -1 ) Fe (mg g -1 ) 188.1 ± 2.8 0.10 ± 0.01 0.023 ± 0.002 To obtain the Mn 2+ and PO 4 3− precursors for the LMP synthesis, the extraction of manganese and residual lithium was carried out by leaching the already water-leached electrodic powder with phosphoric acid. Due to the Mn 4+ insolubility, a reducing agent to form Mn 2+ and/or Mn 3+ was needed. For this purpose, hydrogen peroxide was evaluated as a reducing agent by using two different concentrations of H 3 PO 4 . The H 3 PO 4 concentrations were chosen to respect the stoichiometry of the following reaction: Considering that the dissociation of H 3 PO 4 was dominated by a single dissociation, two acidic solutions were employed. The first solution contained the stoichiometric amount of H + (1.5 M) to react with Mn, while the second solution contained a 100% excess of H + (3 M). Figure 4 shows the effects of the H 3 PO 4 concentration and reducing agent on the Mn and Li extraction. Using 3.0 M phosphoric acid and 20% (v/v) hydrogen peroxide, the maximum yield of Mn extraction was about 75%. It is well known that Mn compounds, such as MnO 2 , as well as activated carbon, can catalyze hydrogen peroxide decomposition to produce water and oxygen (Equations (2) and (3)) [21,22].
Energies 2020, 13, 4004 6 of 11 Energies 2020, 13, x FOR PEER REVIEW 6 of 11 Therefore, to ensure enough reductant was added, an excess of 400% of hydrogen peroxide was employed in the leaching experiments. The use of H2O2 is often a critical issue for the development of a hydrometallurgical process, where its inadvertent decomposition implies a large consumption that could hinder the economic feasibility of the overall process. To avoid the use of H2O2, glucose was further investigated as a reducing agent. The results are reported in Figure S1. The use of glucose was already reported for the extraction of manganese using nitric acid as a leaching agent [23]. On the other hand, the obtained Mn extraction rates using glucose and phosphoric acid were lower than 10%. The H2O2 consumption together with the non-quantitative extraction will need to be studied further to establish more sustainable leaching conditions.

Synthesis and Characterization of LiMnPO4
According to the literature, the minimum reaction time required to obtain LiMnPO4 nanoparticles is only 5 min [24]. Preliminary synthetic experiments were therefore conducted for only five minutes without success. These experiments are not listed below but it was concluded that to obtain LiMnPO4, a longer reaction time is required. The subsequent series of experiments were carried out with different reaction times to evaluate the effect of this parameter on the morphology and size of the obtained products. It was observed that after 30 min, parallelepiped-shaped particles with a length of about 1 micron and a width of 300 nm were obtained. EDX microanalysis (Table S2) also confirmed the presence of manganese and phosphorus, with a stoichiometric ratio close to 1:1, as expected from the theoretical stoichiometry (Li:Mn:P = 1:1:1). Therefore, to ensure enough reductant was added, an excess of 400% of hydrogen peroxide was employed in the leaching experiments. The use of H 2 O 2 is often a critical issue for the development of a hydrometallurgical process, where its inadvertent decomposition implies a large consumption that could hinder the economic feasibility of the overall process. To avoid the use of H 2 O 2 , glucose was further investigated as a reducing agent. The results are reported in Figure S1. The use of glucose was already reported for the extraction of manganese using nitric acid as a leaching agent [23]. On the other hand, the obtained Mn extraction rates using glucose and phosphoric acid were lower than 10%. The H 2 O 2 consumption together with the non-quantitative extraction will need to be studied further to establish more sustainable leaching conditions.

Synthesis and Characterization of LiMnPO 4
According to the literature, the minimum reaction time required to obtain LiMnPO 4 nanoparticles is only 5 min [24]. Preliminary synthetic experiments were therefore conducted for only five minutes without success. These experiments are not listed below but it was concluded that to obtain LiMnPO 4 , a longer reaction time is required. The subsequent series of experiments were carried out with different reaction times to evaluate the effect of this parameter on the morphology and size of the obtained products. It was observed that after 30 min, parallelepiped-shaped particles with a length of about 1 micron and a width of 300 nm were obtained. EDX microanalysis (Table S2) also confirmed the presence of manganese and phosphorus, with a stoichiometric ratio close to 1:1, as expected from the theoretical stoichiometry (Li:Mn:P = 1:1:1).
The samples synthesized for 60 and 120 min were characterized in the same way as the previous sample. The resulting material showed the same morphology and dimensions ( Figure 5). The Mn:P ratio data obtained from the elemental analysis was not sufficient to confirm the obtainment of LiMnPO 4 . Therefore, X-ray diffraction analysis was performed. Since no significant effect due to the duration was found based on the SEM microscopy results, the best candidate for the analysis was the sample obtained after the lower synthesis duration of 30 min (S30). The XRD pattern ( Figure 6) of sample S30 matched the reference pattern for LiMnPO 4 and confirmed the effective production of the characteristic crystalline phase of LMP.
Preliminary synthesis tests starting from the recovered materials were conducted by directly adding solid Li 2 CO 3 to the Mn 2+ -PO 4 3− precursor solution and then the pH was increased to the desired value. This procedure produced a precipitate that was probably composed of manganese carbonates that hindered the formation of LMP. The dissolution of the lithium carbonate in sulphuric acid before adding it to the solution allowed for the elimination of the CO 3 2− anions, causing the evolution of CO 2 , and therefore the precipitation of carbonate was avoided. Figure 6 displays the SEM images of the LMP samples produced using the recovered lithium carbonate and Mn 2+ -PO 4 3− solution. Small particles of about 50 nm, with an atomic ratio Mn:P close to 0.75 (Table S2), were found in the sample with a reaction duration of 30 min (R30) ( Figure 6A). Even in this case, the role of the reaction duration was investigated. The sample obtained after 60 min (R60) of reaction time showed more homogeneous particles with an average size of about 100 nm. By analyzing the areas of the sample in which the particles were clearly visible, the presence of manganese and phosphorus in a ratio close to 0.65 was verified (Table S2). EDX analysis of both the LMP produced by the recovery procedure revealed an excess of phosphorus.
the other hand, the obtained Mn extraction rates using glucose and phosphoric acid were lower than 10%. The H2O2 consumption together with the non-quantitative extraction will need to be studied further to establish more sustainable leaching conditions.

Synthesis and Characterization of LiMnPO4
According to the literature, the minimum reaction time required to obtain LiMnPO4 nanoparticles is only 5 min [24]. Preliminary synthetic experiments were therefore conducted for only five minutes without success. These experiments are not listed below but it was concluded that to obtain LiMnPO4, a longer reaction time is required. The subsequent series of experiments were carried out with different reaction times to evaluate the effect of this parameter on the morphology and size of the obtained products. It was observed that after 30 min, parallelepiped-shaped particles with a length of about 1 micron and a width of 300 nm were obtained. EDX microanalysis (Table S2) also confirmed the presence of manganese and phosphorus, with a stoichiometric ratio close to 1:1, as expected from the theoretical stoichiometry (Li:Mn:P = 1:1:1). The samples synthesized for 60 and 120 min were characterized in the same way as the previous sample. The resulting material showed the same morphology and dimensions ( Figure 5). The Mn:P ratio data obtained from the elemental analysis was not sufficient to confirm the obtainment of LiMnPO4. Therefore, X-ray diffraction analysis was performed. Since no significant effect due to the duration was found based on the SEM microscopy results, the best candidate for the analysis was the sample obtained after the lower synthesis duration of 30 min (S30). The XRD pattern ( Figure 6) of sample S30 matched the reference pattern for LiMnPO4 and confirmed the effective production of the characteristic crystalline phase of LMP. Preliminary synthesis tests starting from the recovered materials were conducted by directly adding solid Li2CO3 to the Mn 2+ -PO4 3− precursor solution and then the pH was increased to the desired value. This procedure produced a precipitate that was probably composed of manganese carbonates that hindered the formation of LMP. The dissolution of the lithium carbonate in sulphuric acid before adding it to the solution allowed for the elimination of the CO3 2− anions, causing the evolution of CO2, and therefore the precipitation of carbonate was avoided. Figure 6 displays the SEM images of the LMP samples produced using the recovered lithium carbonate and Mn 2+ -PO4 3− solution. Small particles of about 50 nm, with an atomic ratio Mn:P close to 0.75 (Table S2), were found in the sample with a reaction duration of 30 min (R30) ( Figure 6A). Even in this case, the role of the reaction duration was investigated. The sample obtained after 60 min (R60) of reaction time showed more homogeneous particles with an average size of about 100 nm. By analyzing the areas of the sample in which the particles were clearly visible, the presence of manganese and phosphorus in a ratio close to 0.65 was verified (Table S2). EDX analysis of both the LMP produced by the recovery procedure revealed an excess of phosphorus. XRD analysis of samples R30 and R60 was performed and the relative patterns are shown in Figure 7. Different to sample S30, both samples R30 and R60 showed the presence of other peaks that were not related to the LMP phase. In particular, samples R30 and R60 showed some characteristics peaks that could be related to the formation of Li 3 PO 4 . Furthermore, the increase of the reaction time to 60 min enabled the formation of Mn 3 O 4 , as revealed by the XRD pattern of the R60 sample. Due to the formation of the Mn 3 O 4 phase, a reaction time of 60 min could not be considered using the reported synthesis method. On the other hand, it is noted that Li 3 PO 4 is a soluble salt that can be easily removed by washing the produced solid. The formation of Li 3 PO 4 could be related to the excess of PO 4 3− and Li contained in the precursor solution. The formation of Li 3 PO 4 could be avoided with the addition of synthetic reagents to reach the desired stoichiometry between Li, Mn, and PO 4 3− . On the other hand, the introduction of primary sources into the proposed process goes beyond the aim of this work.
Energies 2020, 13, 4004 8 of 11 Energies 2020, 13, x FOR PEER REVIEW 8 of 11 Figure 7. XRD spectra of the synthesized LMP and a reference spectra for LMP and Li3PO4.
XRD analysis of samples R30 and R60 was performed and the relative patterns are shown in Figure 7. Different to sample S30, both samples R30 and R60 showed the presence of other peaks that were not related to the LMP phase. In particular, samples R30 and R60 showed some characteristics peaks that could be related to the formation of Li3PO4. Furthermore, the increase of the reaction time to 60 min enabled the formation of Mn3O4, as revealed by the XRD pattern of the R60 sample. Due to the formation of the Mn3O4 phase, a reaction time of 60 min could not be considered using the reported synthesis method. On the other hand, it is noted that Li3PO4 is a soluble salt that can be easily removed by washing the produced solid. The formation of Li3PO4 could be related to the excess of PO4 3− and Li contained in the precursor solution. The formation of Li3PO4 could be avoided with the addition of synthetic reagents to reach the desired stoichiometry between Li, Mn, and PO4 3− . On the other hand, the introduction of primary sources into the proposed process goes beyond the aim of this work.

Mass Balance of the Proposed Process
Data derived from the recovery of Li and Mn, together with the data obtained from the synthesis of the LMP, were employed to compose a preliminary materials balance of the whole proposed process. The amounts of the steel, electrodic powder, and plastics fractions were estimated after the crushing, sieving, and magnetic separation of 300 kg of Li-MnO2 coin-cell batteries. The material mass balance was computed with the following considerations:  The results of the electrodic powder washing showed about half of the total lithium contained in the batteries was present as an insoluble species. The insoluble lithium was considered to be LiMnO2.  The carbon fraction was estimated by subtracting the LiMnO2 and MnO2 amounts remaining in the fine fraction that resulted after water leaching. Here it was assumed that after water washing, the residual insoluble species were carbon, LiMnO2, and MnO2. The LiMnO2 and MnO2 amounts were estimated from the Li and Mn analysis in the washed electrodic powder.  The remainder of the residue was considered to be made up of solvents and organic salts based on the datasheet of the most common coin-cell batteries on the market. The inputs and outputs of the materials from the proposed process are included in the functional flow block diagram reported in Figure 8. Detailed compositions of all streams are given in Table S3. The materials' masses were computed for a batch feed consisting of 100 kg of batteries. The magnetic separation operation performed after the sieving produced for 44 kg of recoverable steel and 18 kg of a nonmagnetic fraction, which was mainly composed of the polypropylene to be separated. A total water supply of about 500 kg was needed to treat a battery batch and will become an amount of liquid waste to dispose at the end of the process. Performing the leaching with phosphoric acid allowed for

Mass Balance of the Proposed Process
Data derived from the recovery of Li and Mn, together with the data obtained from the synthesis of the LMP, were employed to compose a preliminary materials balance of the whole proposed process. The amounts of the steel, electrodic powder, and plastics fractions were estimated after the crushing, sieving, and magnetic separation of 300 kg of Li-MnO 2 coin-cell batteries. The material mass balance was computed with the following considerations: • The results of the electrodic powder washing showed about half of the total lithium contained in the batteries was present as an insoluble species. The insoluble lithium was considered to be LiMnO 2 .

•
The carbon fraction was estimated by subtracting the LiMnO 2 and MnO 2 amounts remaining in the fine fraction that resulted after water leaching. Here it was assumed that after water washing, the residual insoluble species were carbon, LiMnO 2 , and MnO 2 . The LiMnO 2 and MnO 2 amounts were estimated from the Li and Mn analysis in the washed electrodic powder.

•
The remainder of the residue was considered to be made up of solvents and organic salts based on the datasheet of the most common coin-cell batteries on the market.
The inputs and outputs of the materials from the proposed process are included in the functional flow block diagram reported in Figure 8. Detailed compositions of all streams are given in Table S3. The materials' masses were computed for a batch feed consisting of 100 kg of batteries. The magnetic separation operation performed after the sieving produced for 44 kg of recoverable steel and 18 kg of a nonmagnetic fraction, which was mainly composed of the polypropylene to be separated. A total water supply of about 500 kg was needed to treat a battery batch and will become an amount of liquid waste to dispose at the end of the process. Performing the leaching with phosphoric acid allowed for a leachate precursor for the synthesis of 25 kg of LMP to be obtained. Due to the excess of PO 4 3− and Li + in the LMP synthesis streams, a solution with 6 kg of potentially recoverable Li 3 PO 4 was the product at the end of the process. The proposed process, as the major part of the hydrometallurgical processes, used a large amount of water (5 kg of water per kg of treated batteries). The recycling of the water employed when processing the batteries could be advantageous for the sustainability of the process. Regarding the water needed for the neutralization (stream 7- Figure 8), recycling is currently expected. The same water stream can be used for the extraction of lithium in four consecutive batches, as illustrated in Section 2.2. After the recovery of Li 2 CO 3 (stream 17- Figure 8), this solution will be rich in Na and the soluble organic electrolytes contained in the batteries. Characterization of the organic loading of the resulting solution should be addressed to evaluate possible further reuse of this stream. The wastewater coming from the LMP synthesis (stream 21- Figure 8) should contain only unreacted Li and could be recycled for the Li extraction (stream 7- Figure 8). A preliminary cost Energies 2020, 13, 4004 9 of 11 analysis that took into account the reagents' costs and the products' revenues is reported in Table S4. Excluding the energy consumption costs, a positive economic balance of the process was found.
currently expected. The same water stream can be used for the extraction of lithium in four consecutive batches, as illustrated in Section 2.2. After the recovery of Li2CO3 (stream 17- Figure 8), this solution will be rich in Na and the soluble organic electrolytes contained in the batteries. Characterization of the organic loading of the resulting solution should be addressed to evaluate possible further reuse of this stream. The wastewater coming from the LMP synthesis (stream 21- Figure 8) should contain only unreacted Li and could be recycled for the Li extraction (stream 7- Figure 8). A preliminary cost analysis that took into account the reagents' costs and the products' revenues is reported in Table S4. Excluding the energy consumption costs, a positive economic balance of the process was found.

Conclusions
The proposed process is an attractive solution for the treatment of primary Li-MnO2 batteries. These kinds of batteries are not treated with a dedicated process but instead are fed into a pyrometallurgical process with other wastes, resulting in the subsequent loss of Li and Mn. The cryogenic crushing of the batteries has allowed for their mechanical treatment without concern for the safety risks caused by the presence of metallic lithium and flammable electrolytes. Sieving 100 kg of crushed materials resulted in 44 kg of recoverable steel, 18 kg of plastics, and electrodic powder. The electrodic powder was employed as the raw material for the synthesis of LiMnPO4 nanoparticles. Li2CO3 with a purity of 99% was recovered after its precipitation from the lithium-rich solution, which resulted from the washing of the electrodic powder. Leaching the electrodic powder with H3PO4 produced a Mn-bearing solution, which was directly employed for the synthesis of LiMnPO4. The obtained data were employed to compose the materials balance of the process. After treating 100 kg of batteries, 25 kg of LMP and potentially 6 kg of Li3PO4 could be produced. The easy process

Conclusions
The proposed process is an attractive solution for the treatment of primary Li-MnO 2 batteries. These kinds of batteries are not treated with a dedicated process but instead are fed into a pyrometallurgical process with other wastes, resulting in the subsequent loss of Li and Mn. The cryogenic crushing of the batteries has allowed for their mechanical treatment without concern for the safety risks caused by the presence of metallic lithium and flammable electrolytes. Sieving 100 kg of crushed materials resulted in 44 kg of recoverable steel, 18 kg of plastics, and electrodic powder. The electrodic powder was employed as the raw material for the synthesis of LiMnPO 4 nanoparticles. Li 2 CO 3 with a purity of 99% was recovered after its precipitation from the lithium-rich solution, which resulted from the washing of the electrodic powder. Leaching the electrodic powder with H 3 PO 4 produced a Mn-bearing solution, which was directly employed for the synthesis of LiMnPO 4 . The obtained data were employed to compose the materials balance of the process. After treating 100 kg of batteries, 25 kg of LMP and potentially 6 kg of Li 3 PO 4 could be produced. The easy process configuration, together with the production of high-value-added products, could pave the way for the development of a dedicated process for the treatment of Li primary batteries.
Supplementary Materials: The following are available online at http://www.mdpi.com/1996-1073/13/15/4004/s1. Figure S1: Extractive yields of Li and Mn after leaching for 3 h under stirring at 85 • C. Table S1: Lithium concentration trend due to recycling the washing solution. Table S2: Mn, P, and O amounts in the produced LMP samples as estimated using EDX analysis. Table S3: Materials balance in kilograms of the proposed process. Table S4: Preliminary economic analysis of the process considering the operative costs excluding the costs associated with the energy consumption.
Author Contributions: Conceptualization, P.G.S. and F.P.; methodology, F.C.d.S.M.P. and P.G.S.; data curation, P.G.S.; writing-original draft preparation, P.G.S.; writing-review and editing, P.G.S., F.P. and P.A.; funding acquisition, P.A. All authors have read and agreed to the published version of the manuscript.
Funding: Mechanical treatment operations were carried out within the LIFE-LIBAT project (LIFE16 ENV/IT/ 000389).