Many important metals occur as sulfide, arsenide, and antimonide minerals, especially in the Sudbury

Question

mineral complex. The first step in processing these ores involves “roasting” the ore in air to produce the metal
or metal oxide, along with nonmetal oxides that can be serious pollutants if not trapped.
Suppose that you roast 2.00 kg of the mineral marcasite, FeS2. The balanced equation for the reaction is:
4 FeS2 + 11 O2 → 2 Fe2O3 + 8 SO2
(a) How many kg of Fe2O3 can be produced?
(b) How many kg of the pollutant SO2 can be produced?
(c) How many liters of air at 25°C are required for roasting? Assume that air contains 23% O2 by mass,
and that the density of air at 25°C is 1.2 g/L.
Molar masses: FeS2 120.0 g/mol Fe2O3 159.69 g/mol SO2 64.06 g/mol

Answer 1

How much of this do you already know how to do. I don't need to work those parts you know. If you want to post your work I'll look at it up to the point you don't know how to proceed.

Answer 2

I don´t know anything