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The mass percentage of pure Fe2O3 can be computed using the equation:
Since the reaction is 100% efficient this means that all Fe2O3 in the iron ore reacted to form pure Fe.
The mass of impure Fe2O3 or the mass of the iron ore sample is already given as 752 g.
But, the mass of pure Fe2O3 needs to be calculated based on the moles of Fe produced in the reaction.
We can solve for the Mass of Fe2O3 through the following steps:
An iron ore sample contains Fe2O3 plus other impurities. A 752-g sample of impure iron ore is heated with excess carbon, producing 453 g of pure iron by the following reaction:
Fe2O3 (s) + 3 C (s) → 2 Fe (s) + 3 CO (g)
What is the mass percent of Fe 2O3 in the impure iron ore sample? Assume that Fe 2O3 is the only source of iron and that the reaction is 100% efficient.
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Mass Percent Formula concept. You can view video lessons to learn Mass Percent Formula. Or if you need more Mass Percent Formula practice, you can also practice Mass Percent Formula practice problems.
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Based on our data, we think this problem is relevant for Professor Cruz's class at USF.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.