Porous pellets of TiO₂ can be reduced to titanium m...

Question

Porous pellets of TiO₂ can be reduced to titanium metal at the cathode of an electrochemical cell containing molten CaCl₂ as the electrolyte. When the TiO₂ is reduced, the O^2-ions dis-solve in the CaCl₂ and are subsequently oxidized to O₂ gas at the anode. This approach may be the basis for a less expensive process than the one currently used for producing titanium.
(c) Write balanced equations for the anode, cathode, and overall cell reactions.

(c) Write balanced equations for the anode, cathode, and overall cell reactions.

Accepted Answer

insert step 1\u003e Identify the half-reactions occurring at the cathode and anode. At the cathode, $$TiO_2 is $$reduced to titanium metal, and at the anode, $$O^{2-}$$ ions are oxidized to $$O_2$$ gas.. insert step 2\u003e Write the reduction half-reaction at the cathode. $$TiO_2 is $$reduced to Ti metal, so the half-reaction is: $$TiO_2 + 4e^- + 4H$$^+ \rightarrow Ti + 2H_2O.. insert step 3\u003e Write the oxidation half-reaction at the anode. $$O^{2-}$$ ions are oxidized to $$O_2$$ gas, so the half-reaction is: $$2O^{2-}$$ \rightarrow $$O_2 + 4e^-.. $$insert step 4\u003e Balance the electrons in both half-reactions to ensure the number of electrons lost in the oxidation reaction equals the number gained in the reduction reaction.. insert step 5\u003e Combine the balanced half-reactions to write the overall balanced cell reaction.

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Key Concepts

Electrochemical Cells

Oxidation and Reduction

Balancing Redox Reactions