Bioleaching

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Bioleaching is the extraction of metals from their ores through the use of living organisms. This is much cleaner than the traditional heap leaching using cinema.[1] Bioleaching is one of several applications within biohydrometallurgy and several methods are used to recover copper, zinc, lead, arsenic, antimony, nickel, molybdenum, gold, silver, and cobalt.

Process[edit]

Bioleaching can involve numerous ferrous iron and sulfur oxidizing bacteria, including Acidithiobacillus ferrooxidans and Acidithiobacillus (formerly known as Thiobacillus). As a general principle, Fe3+ ions are used to oxidize the ore. This step is entirely independent of microbes. The role of the bacteria is the further oxidation of the ore, but also the regeneration of the chemical oxidant Fe3+ from Fe2+. For example, bacteria catalyse the breakdown of the mineral pyrite (FeS2) by oxidising the sulfur and metal (in this case ferrous iron, (Fe2+)) using oxygen. This yields soluble products that can be further purified and refined to yield the desired metal.

Pyrite leaching (FeS2): In the first step, disulfide is spontaneously oxidized to thiosulfate by ferric ion (Fe3+), which in turn is reduced to give ferrous ion (Fe2+):

(1)   \mathrm{FeS_2 + 6 \ Fe^{\,3+} + 3 \ H_2O \longrightarrow 7 \ Fe^{\,2+} + S_2O_3^{\,2-} + 6 \ H^+}    spontaneous

The ferrous ion is then oxidized by bacteria using oxygen:

(2)   \mathrm{4 \ Fe^{\,2+} + \ O_2 + 4 \ H^+ \longrightarrow 4 \ Fe^{\,3+} + 2 \ H_2O}    (iron oxidizers)

Thiosulfate is also oxidized by bacteria to give sulfate:

(3)   \mathrm{S_2O_3^{\,2-} + 2 \ O_2 + H_2O \longrightarrow 2 \ SO_4^{\,2-} + 2 \ H^+}    (sulfur oxidizers)

The ferric ion produced in reaction (2) oxidized more sulfide as in reaction (1), closing the cycle and given the net reaction:

(4)  \mathrm{2 \ FeS_2 + 7 \ O_2 + 2 \ H_2O \longrightarrow 2 \ Fe^{\,2+} + 4 \ SO_4^{\,2-} + 4 \ H^+}

The net products of the reaction are soluble ferrous sulfate and sulfuric acid.

The microbial oxidation process occurs at the cell membrane of the bacteria. The electrons pass into the cells and are used in biochemical processes to produce energy for the bacteria while reducing oxygen to water. The critical reaction is the oxidation of sulfide by ferric iron. The main role of the bacterial step is the regeneration of this reactant.

The process for copper is very similar, but the efficiency and kinetics depend on the copper mineralogy. The most efficient minerals are supergene minerals such as chalcocite, Cu2S and covellite, CuS. The main copper mineral chalcopyrite (CuFeS2) is not leached very efficiently, which is why the dominant copper-producing technology remains flotation, followed by smelting and refining. The leaching of CuFeS2 follows the two stages of being dissolved and then further oxidised, with Cu2+ ions being left in solution.

Chalcopyrite leaching:

(1)   \mathrm{CuFeS_2 + 4 \ Fe^{\,3+} \longrightarrow Cu^{\,2+} + 5 \ Fe^{\,2+} + 2 \ S_0}    spontaneous
(2)   \mathrm{4 \ Fe^{\,2+} + O_2 + 4 \ H^+ \longrightarrow 4 \ Fe^{\,3+} + 2 \ H_2O}    (iron oxidizers)
(3)   \mathrm{2 \ S^0 + 3 \ O_2 + 2 \ H_2O \longrightarrow 2 \ SO_4^{\,2-} + 4 \ H^+}    (sulfur oxidizers)

net reaction:

(4)  \mathrm{CuFeS_2 + 4 \ O_2 \longrightarrow Cu^{\,2+} + Fe^{\,2+} + 2 \ SO_4^{\,2-}}

In general, sulfides are first oxidized to elemental sulfur, whereas disulfides are oxidized to give thiosulfate, and the processes above can be applied to other sulfidic ores. Bioleaching of non-sulfidic ores such as pitchblende also uses ferric iron as an oxidant (e.g., UO2 + 2 Fe3+ ==> UO22+ + 2 Fe2+). In this case, the sole purpose of the bacterial step is the regeneration of Fe3+. Sulfidic iron ores can be added to speed up the process and provide a source of iron. Bioleaching of non-sulfidic ores by layering of waste sulfides and elemental sulfur, colonized by Acidithiobacillus spp., has been accomplished, which provides a strategy for accelerated leaching of materials that do not contain sulfide minerals.[2]

Further processing[edit]

The dissolved copper (Cu2+) ions are removed from the solution by ligand exchange solvent extraction, which leaves other ions in the solution. The copper is removed by bonding to a ligand, which is a large molecule consisting of a number of smaller groups, each possessing a lone electron pair. The ligand-copper complex is extracted from the solution using an organic solvent such as kerosene:

Cu2+(aq) + 2LH(organic) → CuL2(organic) + 2H+(aq)

The ligand donates electrons to the copper, producing a complex - a central metal atom (copper) bonded to the ligand. Because this complex has no charge, it is no longer attracted to polar water molecules and dissolves in the kerosene, which is then easily separated from the solution. Because the initial reaction is reversible, it is determined by pH. Adding concentrated acid reverses the equation, and the copper ions go back into an aqueous solution.

Then the copper is passed through an electro-winning process to increase its purity: An electric current is passed through the resulting solution of copper ions. Because copper ions have a 2+ charge, they are attracted to the negative cathodes and collect there.

The copper can also be concentrated and separated by displacing the copper with Fe from scrap iron:

Cu2+(aq) + Fe(s) → Cu(s) + Fe2+(aq)

The electrons lost by the iron are taken up by the copper. Copper is the oxidising agent (it accepts electrons), and iron is the reducing agent (it loses electrons).

Traces of precious metals such as gold may be left in the original solution. Treating the mixture with sodium cyanide in the presence of free oxygen dissolves the gold. The gold is removed from the solution by adsorbing (taking it up on the surface) to charcoal.

Bioleaching with fungi[edit]

Several species of fungi can be used for bioleaching. Fungi can be grown on many different substrates, such as electronic scrap, catalytic converters, and fly ash from municipal waste incineration. Experiments have shown that two fungal strains (Aspergillus niger, Penicillium simplicissimum) were able to mobilize Cu and Sn by 65%, and Al, Ni, Pb, and Zn by more than 95%.Aspergillus niger can produce some organic acids such as citric acid. This form of leaching does not rely on microbial oxidation of metal but rather uses microbial metabolism as source of acids that directly dissolve the metal.

Compared with other extraction techniques[edit]

Extractions involve many expensive steps such as roasting and smelting, which require sufficient concentrations of elements in ores and are environmentally unfriendly. Low concentrations are not a problem for bacteria because they simply ignore the waste that surrounds the metals, attaining extraction yields of over 90% in some cases. These microorganisms actually gain energy by breaking down minerals into their constituent elements. The company simply collects the ions out of the solution after the bacteria have finished. There is a limited amount of ores.

Advantages of bioleaching[edit]

Disadvantages of bioleaching[edit]

At the current time, it is more economical to smelt copper ore rather than to use bioleaching, since the concentration of copper in its ore is in general quite high. The profit obtained from the speed and yield of smelting justifies its cost. Nonetheless, at the largest copper mine of the world, Escondida in Chile the process seems to be favorable. However, the concentration of gold in its ore is in general very low. The lower cost of bacterial leaching in this case outweighs the time it takes to extract the metal. Economically it is also very expensive and many companies once started can not keep up with the demand and end up in debt. Projects like Finnish Talvivaara proved to be environmentally and economically disastrous.

See also[edit]

References[edit]

  1. ^ "Flotation technique cleaner than heap leaching". Ngm.nationalgeographic.com. 2012-05-15. Retrieved 2012-10-04. 
  2. ^ Power, I.M., Dipple, G.M., and Southam, G. (2010) Bioleaching of ultramafic tailings by Acidithiobacillus spp. for CO2 sequestration, http://pubs.acs.org/doi/abs/10.1021/es900986n Environmental Science & Technology. 44: 456-462.

Further reading[edit]