Titanium is extracted from titanium dioxide using the Hunter process in a two-stage industrial method.
Stage 1 $\quad
\text{TiO}_2 + 2\text{C} + 2\text{Cl}_2 \rightarrow \text{TiCl}_4 + 2\text{CO}$ **Stage 2** $\quad\text{TiCl}_4 + 4\text{Na} \rightarrow \text{Ti} + 4\text{NaCl}$
Suggest one hazard associated with Stage 1.
Suggest why the reaction in Stage 2 is carried out in an atmosphere of argon and not in air.
Titanium chloride (TiCl4\text{TiCl}_4TiCl4) is a liquid at room temperature. Explain why you would not expect a transition metal chloride to be a liquid at room temperature.
During Stage 2, sodium atoms are oxidised to sodium ions. Complete the half-equation for this oxidation. Na→Na++‾\text{Na} \rightarrow \text{Na}^{+} + \underline{\qquad\qquad}Na→Na++
In Stage 2, 47.5 kg47.5\text{ kg}47.5 kg of titanium chloride was added to 25.0 kg25.0\text{ kg}25.0 kg of sodium. Relative atomic masses (ArA_rAr): Na=23\text{Na} = 23Na=23, Cl=35.5\text{Cl} = 35.5Cl=35.5, Ti=48\text{Ti} = 48Ti=48 Explain why titanium chloride is the limiting reactant. You must show your working.
For a Stage 2 reaction, the percentage yield of titanium was 84.5%84.5\%84.5%. The theoretical maximum mass of titanium produced in this batch was 18.5 kg18.5\text{ kg}18.5 kg. Calculate the actual mass of titanium produced. Give your answer to 3 significant figures.