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Iron pyrite is roasted in air: 4FeS2 + 11O2 -> 2Fe2O3 + 8SO2. All the…
Question
Iron pyrite is roasted in air: 4FeS2 + 11O2 -> 2Fe2O3 + 8SO2. All the SO2 produced is then catalytically oxidized to SO3 and absorbed in water to form sulphuric acid, with each SO2 ultimately giving one H2SO4 (molar mass 98). Starting from 120 g of FeS2 (molar mass 120) and assuming 100% conversion at every stage, calculate the mass (in g) of H2SO4 produced.
✓ Verified answer: 196checked by our engine — not a guess
Step-by-step solution
Moles FeS2 = 120/120 = 1.00.
From 4FeS2 -> 8SO2, moles SO2 = (8/4) x 1.00 = 2.00.
Each SO2 -> SO3 -> H2SO4 (1:1), so moles H2SO4 = 2.00.
Mass H2SO4 = 2.00 x 98 = 196 g.
Final answer196.0
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