Asked by lilly
heating an ore of antimony and iron II sulfide.
Sb2S3+3Fe-->2Sb+3FeS
when 15g Sb2S3 reacts with an excess of Fe, 9.84g Sb is produced. what is the pecent yeild of this reaction?
Sb2S3+3Fe-->2Sb+3FeS
when 15g Sb2S3 reacts with an excess of Fe, 9.84g Sb is produced. what is the pecent yeild of this reaction?
Answers
Answered by
DrBob222
Convert 15 g Sb2S3 to mols using mols = g/molar mass.
Convert mols Sb2S3 to mols mols Sb using the coefficients in the balanced equation.
Convert mols Sb to grams using g = mols x molar mass. This is the theoretical yield.
%yield = [(actual yield)/(theoretical yield)]*100
actual yield is 9.84 g.
theoretical yield is calculated above.
Convert mols Sb2S3 to mols mols Sb using the coefficients in the balanced equation.
Convert mols Sb to grams using g = mols x molar mass. This is the theoretical yield.
%yield = [(actual yield)/(theoretical yield)]*100
actual yield is 9.84 g.
theoretical yield is calculated above.
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