Sulfuric acid can be manufactured from hydrogen sulfide in a three-stage process.
stage 1: hydrogen sulfide is burned in oxygen to form sulfur dioxide and steam
2H2S+3O2→2SO2+2H2O 2\text{H}_2\text{S} + 3\text{O}_2 \rightarrow 2\text{SO}_2 + 2\text{H}_2\text{O} 2H2S+3O2→2SO2+2H2Ostage 2: the sulfur dioxide is reacted with more oxygen to form sulfur trioxide
2SO2+O2→2SO3 2\text{SO}_2 + \text{O}_2 \rightarrow 2\text{SO}_3 2SO2+O2→2SO3stage 3: the sulfur trioxide is reacted with concentrated sulfuric acid to form oleum (H2S2O7\text{H}_2\text{S}_2\text{O}_7H2S2O7), which is then reacted with water to form sulfuric acid.
Write a chemical equation for the reaction in stage 3 where oleum (H2S2O7\text{H}_2\text{S}_2\text{O}_7H2S2O7) reacts with water to form sulfuric acid (H2SO4\text{H}_2\text{SO}_4H2SO4).
A mass of 68 tonnes68\text{ tonnes}68 tonnes of hydrogen sulfide is reacted with oxygen in stage 1.
Calculate the maximum mass, in tonnes, of sulfur trioxide (SO3\text{SO}_3SO3) that can be produced in stage 2.
1 tonne=1.0×106 g 1\text{ tonne} = 1.0 \times 10^6\text{ g} 1 tonne=1.0×106 g Relative atomic masses: H=1, O=16, S=32 \text{Relative atomic masses: } H = 1, \text{ } O = 16, \text{ } S = 32 Relative atomic masses: H=1, O=16, S=32Calculate the minimum volume at rtp, in cubic decimetres (dm3\text{dm}^3dm3), of oxygen required to completely react with 96 tonnes96\text{ tonnes}96 tonnes of sulfur dioxide in stage 2.
1 mol of gas at rtp has a volume of 24 dm3 1\text{ mol of gas at rtp has a volume of } 24\text{ dm}^3 1 mol of gas at rtp has a volume of 24 dm3
