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Chapter 21: Problem 15

Starting with rutile \(\left(\mathrm{TiO}_{2}\right),\) explain how you would obtain pure titanium metal. (Hint: First convert \(\mathrm{TiO}_{2}\) to \(\mathrm{TiCl}_{4} .\) Next, reduce \(\mathrm{TiCl}_{4}\) with \(\mathrm{Mg}\). Look up physical properties of \(\mathrm{TiCl}_{4}, \mathrm{Mg},\) and \(\mathrm{MgCl}_{2}\) in a chemistry handbook.)

Short Answer

Expert verified
Initially, \(\mathrm{TiO}_{2}\) is converted to \(\mathrm{TiCl}_{4}\) by heating with chlorine. Then, \(\mathrm{TiCl}_{4}\) is reduced by magnesium, producing pure titanium and magnesium chloride. The reaction is carried out in an argon atmosphere at high temperature. The product mix is then allowed to cool, and magnesium & magnesium chloride - which are highly volatile, are removed easily, leaving behind pure titanium.

Step by step solution

01

- Conversion of Titanium Dioxide to Titanium Tetrachloride

We first react the titanium dioxide with chlorine. With heating, we get titanium tetrachloride and oxygen. The reaction can be given by \[\mathrm{TiO}_{2} + 2\mathrm{Cl}_{2} \longrightarrow \mathrm{TiCl}_{4} + O_{2}\] This formed titanium tetrachloride is a colorless distillable liquid that boils at 136.4 degrees Celsius.
02

- Reduction of Titanium Tetrachloride

We then reduce the titanium tetrachloride by heating it with magnesium. This will yield pure titanium and magnesium chloride. The reaction is \[\mathrm{TiCl}_{4} + 2\mathrm{Mg} \longrightarrow \mathrm{Ti} + 2 \mathrm{MgCl}_{2}\] This reaction is carried out in an argon atmosphere at 800 – 850 °C.
03

- Isolation of pure Titanium

The product from step 2 is allowed to cool. Magnesium and magnesium chloride can be easily removed from the reaction mixture, as they are quite volatile, leaving behind pure Titanium metal. Magnesium can be recycled from magnesium chloride through the electrolysis process.

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Most popular questions from this chapter

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