Exercise - Equation Stoichiometry with Mixtures:
The FeS2 found in pyrite ore is a source of sulfur for the
production of sulfuric acid. In a series of three reactions, the sulfur in FeS2
is converted to sulfur dioxide, which in turn is converted to sulfur trioxide,
which forms sulfuric acid when added to water:
11O2 2Fe2O3 +
a. If, as the first step in this process, 2.75 Mg of pyrite ore that
is 92.6% FeS2 is reacted with excess oxygen in air, what is the
maximum mass of iron(III) oxide, Fe2O3, that can be
the pyrite ore is 92.6% FeS2, what is the minimum mass of ore
necessary to produce 1.00 Mg of iron(III) oxide, Fe2O3?
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