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 the 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 23.3% Ti by mass is digested with an 80.0% H2SO4 solution, supplied in 60.0% 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 92.0% of the ilmenite actually decomposes. Calculate the masses (kg) of ore and 80.0% sulfuric acid solution that must be fed to produce 1000 kg of pure TiO2. kg ore kg 80.0% H2SO4
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 the 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 23.3% Ti by mass is digested with an 80.0% H2SO4 solution, supplied in 60.0% 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 92.0% of the ilmenite actually decomposes. Calculate the masses (kg) of ore and 80.0% sulfuric acid solution that must be fed to produce 1000 kg of pure TiO2. kg ore kg 80.0% H2SO4
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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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 the 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 23.3% Ti by mass is digested with an 80.0% H2SO4 solution, supplied in 60.0% 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 92.0% of the ilmenite actually decomposes. Calculate the masses (kg) of ore and 80.0% sulfuric acid solution that must be fed to produce 1000 kg of pure TiO2.
Suppose an ore containing 23.3% Ti by mass is digested with an 80.0% H2SO4 solution, supplied in 60.0% 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 92.0% of the ilmenite actually decomposes. Calculate the masses (kg) of ore and 80.0% sulfuric acid solution that must be fed to produce 1000 kg of pure TiO2.
kg ore
kg 80.0% H2SO4
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