Difference between revisions of "Iron pyrite"

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In contact with a wet natural environment (water, air, perhaps sunlight), pyrite weathers producing ferrous (and perhaps ferric) sulfates:
 
In contact with a wet natural environment (water, air, perhaps sunlight), pyrite weathers producing ferrous (and perhaps ferric) sulfates:
 
  {{#Chem: 4FeS2(s) + 14O2(g) + 4H2O(l)  =  4Fe<sup>II</sup> + 8SO4<sup>2-</sup> + 8H<sup>+</sup>}}
 
  {{#Chem: 4FeS2(s) + 14O2(g) + 4H2O(l)  =  4Fe<sup>II</sup> + 8SO4<sup>2-</sup> + 8H<sup>+</sup>}}
  {{#Chem: 4Fe<sup>II</sup> + O2 + 4H<sup>+</sup> =  4Fe<sup>III</sup> + 2H2O}}
+
  {{#Chem: 4Fe<sup>II</sup> + O2 + 2H2 =  4Fe<sup>III</sup> + 2H2O}}
 
  {{#Chem: 4Fe<sup>III</sup> + 12 H2O  =    4Fe(OH)3 + 12H<sup>+</sup>}}
 
  {{#Chem: 4Fe<sup>III</sup> + 12 H2O  =    4Fe(OH)3 + 12H<sup>+</sup>}}

Latest revision as of 18:32, 2 October 2019

Iron pyrite 
Frequency common 
Hardness 6-6.5 
Density 5
Chemical Formula FeS2 
Core Elements Fe 
Thermal Decomposition
FeS2
540-850°C
Fe2O3

pyrite, along with Hematite and Magnetite is a primary ore of iron.

Weathering

In contact with a wet natural environment (water, air, perhaps sunlight), pyrite weathers producing ferrous (and perhaps ferric) sulfates:

4 FeS2(s) + 14 O2(g) + 4 H2O(l)  4 FeII + 8 SO42 - + 8 H + 
4 FeII + O2 + 2 H2  4 FeIII + 2 H2O
4 FeIII + 12 H2O  4 Fe(OH)3 + 12 H +