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Iron Sulfide Oxidation as Influenced by Calcium Carbonate Application

L. R. Hossner*,a and J. J. Doolittleb

a Dep. of Soil and Crop Sciences, Texas A&M Univ., College Station, TX 77843
b Plant Science Dep., South Dakota State Univ., Brookings, SD 57007



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Fig. 1. Residual FeS2 and CaCO3 in 1.9% FeS2 overburden treated with CaCO3 to neutralize 0 or 100% of the acid–base account deficit (A/Ba).

 


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Fig. 2. First-order plot of the loss of FeS2 in the 1.9% FeS2 overburden treated with CaCO3 to neutralize 0% of the acid–base account deficit.

 


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Fig. 3. Zero-order (0–100 d) and first-order (100–378 d) plots of the loss of FeS2 in the 4.1% FeS2 overburden treated with CaCO3 to neutralize 25% of the acid–base account deficit.

 


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Fig. 4. Zero-order plot of the loss of FeS2 in the 4.1% FeS2 overburden treated with CaCO3 to neutralize 50, 75, 100, and 125% of the acid–base account deficit (% A/Ba).

 


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Fig. 5. Dissolution rate of CaCO3 in the 4.1% FeS2 overburden treated with CaCO3 to neutralize 25, 50, 75, 100, and 125% of the acid–base account deficit (A/Ba).

 


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Fig. 6. Scanning electron micrographs of representative weathered pyrite particles separated from the overburden following 378 d of incubation and initially containing 4.1% FeS2. (A) Weathered pyrite particle from the 25% acid–base account deficit treatment. (B) Weathered pyrite particle from the 0% acid–base account deficit treatment. (C) Large weathered pyrite particle from the 25% acid–base account deficit treatment. (D) Large pyrite particle from the 125% acid–base account deficit treatment. There is no apparent evidence of pitting and the morphology is similar to pyrite particles at time zero.

 





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