The roasting of nickel sulfide ore (NiS) produces SO2 as one of its products. Ca

Question

The roasting of nickel sulfide ore (NiS) produces SO2 as one of its products. Calculate the volume of SO2, at 25 0C and 1.00 atm, produced by the heat treatment of 10.00 t (10,000 kg) of NiS. What mass of pure H2SO4 could be produced from this amount of SO2?

Explanation / Answer

NiS + 1.5 O2 ---> SO2 + NiO 10,000 kg NIS = 10,000,000/90.7854 = 110149.9 moles SO2 moles = 110149.9 V = nRT/P = 110149.9 x0.0821 x298/1 =2694905 volume of SO2 = 22.4 x 110149.9 = 2694905 liters moles of H2SO4 = 110149.9 mass of H2SO4 = 110149.9 x98.08 = 10.8 tones

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