How is sulfuric acid produced in mine drainage? Write the correspondingstoichiometric equations
Question
How is sulfuric acid produced in mine drainage? Write the correspondingstoichiometric equations
Solution
Sulfuric acid is produced in mine drainage through a series of chemical reactions involving pyrite (FeS2), a common mineral found in rocks. The process is often accelerated by the activity of certain bacteria, such as Acidithiobacillus ferrooxidans.
Here are the steps:
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Pyrite reacts with water and oxygen to form ferrous iron and sulfate. The chemical equation for this reaction is:
4FeS2(s) + 15O2(g) + 14H2O(l) → 4Fe2+(aq) + 8SO42-(aq) + 16H+(aq)
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The ferrous iron produced in the first step can be further oxidized to ferric iron by bacteria:
4Fe2+(aq) + O2(g) + 4H+(aq) → 4Fe3+(aq) + 2H2O(l)
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The ferric iron can then react with more pyrite to produce additional ferrous iron, sulfate, and acidity:
FeS2(s) + 14Fe3+(aq) + 8H2O(l) → 15Fe2+(aq) + 2SO42-(aq) + 16H+(aq)
These reactions result in the production of sulfuric acid (H2SO4), which is responsible for the acidity of mine drainage. The overall reaction can be written as:
2FeS2(s) + 7O2(g) + 2H2O(l) → 2Fe2+(aq) + 4SO42-(aq) + 4H+(aq)
The H+ ions combine with water to form H3O+ ions, which are responsible for the acidity of the solution:
H+(aq) + H2O(l) → H3O+(aq)
This is a simplified explanation and the actual process can be more complex, involving a variety of other reactions and species.
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