Asked by snow
A commercial sample of pyrite (FeS2) is oxidized by bromine and nitric acid. The sulphate obtained is precipitated and heavy in the form of BaSO4. If 0, 331g of pyrite originated 0.813 g of BaSO4, what is the% of sulphur in the studied pyrite? What is the% of FeS2??
Answers
Answered by
DrBob222
g FeS2 = 0..813 g BaSO4 x (molar mass FeS2/2*molar mass BaSO4) = ?. The is the actual yield (AY) of FeS2. Mass sample is 0.331 g.
%yield = (AY/mass sample)*100 = ?
%yield = (AY/mass sample)*100 = ?
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