Final answer:
To calculate the amount of the mineral CaTiO3 required to produce 5.00 tons of titanium, we would need to consider the chemical reactions and limits involved in the extraction process and apply stoichiometry to equate the mass of CaTiO3 to titanium yield. However, insufficient data on the conversion from CaTiO3 to titanium metal makes it impossible to provide a precise answer.
Step-by-step explanation:
The question relates to determining the amount of a titanium-containing mineral required to produce a certain mass of titanium metal. We are given information about the chemistry involved in the extraction process, including details about limiting reactants and reactions involving titanium tetrachloride (TiCl4) and magnesium (Mg).
Given that 197 g of titanium metal is produced from 1.00 kg of titanium tetrachloride and 200 g of magnesium in a particular reaction, we can calculate the amount of the mineral CaTiO3 needed to produce 5.00 tons of titanium. Since magnesium is the limiting reactant in the relevant chemical reactions, we would first determine the amount of magnesium needed to produce 5.00 tons of titanium and then work backwards to find the mass of CaTiO3 that would yield the necessary amount of titanium tetrachloride.
However, since the provided excerpts indicate that titanium tetrachloride is formed from TiO2 and not directly from the mineral CaTiO3, and we do not have information on how to convert CaTiO3 to TiO2 directly, we cannot perform this calculation without further details. Normally, one would follow a series of chemical reactions from the ore to the titanium tetrachloride, and then to the metallic titanium, applying stoichiometry at each step to account for the yield and purity at each stage.