Asked by Chris
A 0.5962g sample of iron ore is dissolved in acid producing Fe3+. Through a series of reactions, the iron precipitates as the Fe(OH)3. The precipitate is heated, forming solid Fe2O3. What is the mass % of iron in the sample if the analysis produced 0.3210g Fe2O3?
Answers
Answered by
MathMate
atomic mass of iron, Fe = 55.845 g/mol
molar mass of Fe2O3 = 159.69 g/mol
Iron content in sample of Fe2O3
= 0.3210*(55.845/159.69)
= 0.11226 g
Percentage of iron in ore
= 0.11226 g/ 0.5962 g
= 18.83%
molar mass of Fe2O3 = 159.69 g/mol
Iron content in sample of Fe2O3
= 0.3210*(55.845/159.69)
= 0.11226 g
Percentage of iron in ore
= 0.11226 g/ 0.5962 g
= 18.83%
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.