Porous pellets of TiO 2 can be reduced to titanium metal at the cathode of an electrochemical cell containing molten CaCl 2 as the electrolyte. When the TiO 2 is reduced, the O 2- ions dis-solve in the CaCl 2 and are subsequently oxidized to O 2 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.

Hello. In this problem, we are told that molten sodium chloride can be reduced to sodium metal are passing an electric current through the molten salt to split it into its elements illustrated below is a simple diagram of the cell. We are asked to show the balanced equations for the anodes, the cathode and the overall cell reactions. So beginning then with the anodes. So recall that oxidation occurs at the anodes. So we will have oxidation then of our paradigms warm flooring gas and we see this taking place in this annual compartment, Floridians are being attracted towards the anodes where they are then oxidized form chlorine gas. We have an inert electrode so that it won't react with our highlight and we need a metal surface. In order for this reaction to occur. We then look at the cathode cathode calls where reduction takes place. So we will have then the reduction of our sodium ions form sodium metal. And so in the cathode compartment we have sodium mines being attracted to the electrode where reduction takes place again, we have an inert electrode. So in this case we have sodium as a liquid. So we need a metal solid. If we combine these two half reactions, we come up with the overall reaction in order to bind them, the number of electrons that are being lost has equal number of electrons being gained. So we'll take the reaction taking place at the cathode and multiply through by two and doing so then our moles of electrons will cancel. And then we're left with two moles of Short irons reacting with two moles of study minds. To give us chlorine gas and sodium metal. You can combine then our sodium and chloride eines. We have two moles of then molten sodium chloride point form pouring gas and sodium metal. So our overall reaction taking place at the anodes is then the oxidation of Floridians reaction taking place at the cathode is the reduction of our sodium minds to form sodium metal, and the overall reaction then, is the molten sodium chloride being converted to chlorine gas and sodium metal. Thanks for watching. Hope this helps.

Ch.19 - Electrochemistry

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

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McMurry 8th Edition

Ch.19 - Electrochemistry

Problem 40c

Chapter 19, Problem 40c

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.

Verified step by step guidance

insert step 1> 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> 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> 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> 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> Combine the balanced half-reactions to write the overall balanced cell reaction.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electrochemical Cells

Electrochemical cells are devices that convert chemical energy into electrical energy through redox reactions. They consist of two electrodes: the anode, where oxidation occurs, and the cathode, where reduction takes place. Understanding the flow of electrons and the movement of ions in these cells is crucial for writing balanced equations for the reactions involved.

Oxidation and Reduction

Oxidation and reduction are fundamental concepts in chemistry that describe the transfer of electrons between species. Oxidation involves the loss of electrons, while reduction involves the gain of electrons. In the context of the electrochemical cell described, the TiO2 is reduced at the cathode, and the O2- ions are oxidized at the anode, which is essential for balancing the overall cell reaction.

Balancing Redox Reactions

Balancing redox reactions requires ensuring that the number of electrons lost in oxidation equals the number gained in reduction. This involves identifying the oxidation states of the elements involved and adjusting coefficients in the half-reactions to achieve mass and charge balance. Mastery of this concept is necessary to write accurate balanced equations for the anode, cathode, and overall reactions in the electrochemical cell.