Draw the reaction scheme for the process and calculate the masses(kg) of ore 80% sulfuric acid solution that must be fed to produce 1000 kg of pure TiO2

Problem 3: 2 pts Titanium dioxide (TiO2) is used extensively as a white pigment. It is produced from an ore that contains ilmenite (FeTiO3) and ferric oxide (Fe2O3). The ore is digested with an aqueous sulfuric acid solution to produce an aqueous solution of titanyl sulfate [(TiO)SO4] and ferrous sulfate (FeSO4). Water is added to hydrolyze the titanyl sulfate to H2TiO3, which precipitates, and H2SO4. The precipitate is then roasted, driving off water and leaving a residue of pure titanium dioxide. (Several steps to remove iron from the intermediate solutions as iron sulfate have been omitted from this description.) Suppose an ore containing 24.3% Ti by mass is digested with an 80% (by mass) H2SO4 solution, supplied in 50% excess of the amount needed to convert all the ilmenite to titanyl sulfate and all the ferric oxide to ferric sulfate [Fe2(SO4)3]. Further suppose that 89% of the ilmenite actually decomposes. Draw the reaction scheme for this process. Calculate the masses (kg) of ore and 80% sulfuric acid solution that must be fed to produce 1000kg of pure TiO2. The reaction scheme is below: FeTiO3+2H2SO4(TiO)SO4+FeSO4+2H2OFe2O3+3H2SO4Fe2(SO4)3+3H2O(TiO)SO4+2H2OH2TiO3(s)+H2SO4H2TiO3(s)TiO2(s)+H2O