Starting with rutile ( TiO2 ), explain how you would obtain pure titanium metal. (Hint: First co

step 1 18 from chapter 23 and it's asking how do we obtain pure titanium dioxide? So the first thing I

Starting with rutile ( TiO2 ), explain how you would obtain...

Starting with rutile ( $\mathrm{TiO}_2$ ), explain how you would obtain pure titanium metal. (Hint: First convert $\mathrm{TiO}_2$ to $\mathrm{TiCl}_4$. Next, reduce $\mathrm{TiCl}_4$ with Mg . Look up physical properties of $\mathrm{TiCl}_4, \mathrm{Mg}$, and $\mathrm{MgCl}_2$ in a chemistry handbook.)

A titanium ore contains rutile $\left(\mathrm{TiO}_{2}\right)$ plus some iron oxide and silica. When it is heated with carbon in the presence of chlorine, titanium tetrachloride, $\mathrm{TiCl}_{4},$ is formed. $$ \mathrm{TiO}_{2}(s)+\mathrm{C}(s)+2 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{TiCl}_{4}(g)+\mathrm{CO}_{2}(g) $$ Titanium tetrachloride, a liquid, can be distilled from the mixture. If $35.4 \mathrm{~g}$ of titanium tetrachloride is recovered from $18.1 \mathrm{~g}$ of crude ore, what is the mass percentage of $\mathrm{TiO}_{2}$ in the ore (assuming all $\mathrm{TiO}_{2}$ reacts)?

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