Sulfuric acid can be manufactured from sulfur in a three-stage industrial process.
stage 1: sulfur is burned in oxygen to form sulfur dioxide
S+O2→SO2 \text{S} + \text{O}_2 \rightarrow \text{SO}_2 S+O2→SO2stage 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 water to form sulfuric acid
Write a chemical equation for the reaction of stage 3 that forms sulfuric acid (H2SO4\text{H}_2\text{SO}_4H2SO4) from sulfur trioxide (SO3\text{SO}_3SO3) and water (H2O\text{H}_2\text{O}H2O).
A mass of 80 tonnes80\text{ tonnes}80 tonnes of sulfur 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]Calculate the minimum volume at rtp, in cubic decimetres (dm3\text{dm}^3dm3), of oxygen required to completely react with 160 tonnes160\text{ tonnes}160 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]
