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Suppose you roast 2.00kg of Fe3S4. The equation:

4Fe3S4 + 25 O2 --> 6Fe2O3 + 16SO2.

a) How many kg of Fe2O3 will be produced?

b) How many kg of SO2 will be produced?

c) How many litres of air at 25 degrees C are required for roasting? Assuming air has 23% O2 by mass, and density of 25C is 1.2 g/L.

The molar masses are Fe3S4 = 295.8 g/mol, Fe2O3 = 159.69 g/mol and SO2 is 64.06 g/mol.

I have done a and b.

a) = 1.62kg

b) = 1.73kg.

I have NO IDEA how to do C! Please guide!

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# Homework Help: Third part to a stoichiometry question

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