A works roasts 600 kg of iron pyrites ore that is 80 % FeS2 by mass…
Contributed by StemPy LabTry it on paper first. A hint, the key idea and the worked solution are here when you need them.
A works roasts of iron pyrites ore that is FeS2 by mass. The reaction is . Take the molar masses as FeS2 , SO2 and Fe2O3 , and the molar volume as at and . Find the mass of sulphur dioxide, its volume, and the mass of iron(III) oxide that remains.
Need a reminder? The key ideaShow
Ozone gives one mole of iodine for each mole of ozone with potassium iodide. Roasting pyrites follows 4FeS2 + 11O2 giving 2Fe2O3 + 8SO2, so each FeS2 gives 2 SO2. Permanganate and dichromate oxidise sulphur dioxide: 5 SO2 for each 2 and 3 SO2 for each . Work in moles: the amount of a solute is the volume in litres times the concentration.
The worked solution
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Work it out on paper first. It is fine to get stuck or make a mistake: that is how we learn. When you are ready, go through the solution one step at a time, and check each step against your own.
Step 1. Pure FeS2. . In kilomoles: .
Step 2. Sulphur dioxide. 4 mol of FeS2 give 8 mol of SO2, so . The mass is .
Step 3. Volume. .
Step 4. Iron(III) oxide. 4 mol of FeS2 give 2 mol of Fe2O3, so . The mass is .
Answer: of SO2, and of Fe2O3.
Check. The sulphur is kept: of S in SO2 equals of S in FeS2.
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