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Chapter 21: Q21.2P (page 972)
Why must an electrochemical process involve a redox reaction?
Because electrons require a source and recipient (in the form of reducing and oxidizing substances) for an electrochemical reaction to occur, redox reactions are used in electrochemical processes.
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How is a standard reference electrode used to determine unknown half-cell values?
Consider the following voltaic cell
(a) In which direction do electrons flow in the external circuit?
(b) In which half-cell does oxidation occur?
(c) In which half-cell do electrons enter the cell?
(d) At which electrode are electrons consumed?
(e) Which electrode is negatively charged?
(f) Which electrode decreases in mass during cell operation?
(g) Suggest a solution for the cathode electrolyte.
(h) Suggest a pair of ions for the salt bridge.
(i) For which electrode could you use an inactive material?
(j) In which direction do anions within the salt bridge move to maintain charge neutrality?
(k) Write balanced half-reactions and an overall cell reaction.
Electrolysis of molten is the final production step in the isolation of magnesium from seawater by the Dow process. Assuming that of metal forms,
(a) How many moles of electrons are required?
(b) How many coulombs are required?
(c) How many amps will produce this amount in?
When a piece of metal A is placed in a solution containing ions of metal , metal plates out on the piece of A.
(a) Which metal is being oxidized?
(b) Which metal is being displaced?
(c) Which metal would you use as the anode in a voltaic cell incorporating these two metals?
(d) If bubbles of form when is placed in acid, will they form if A is placed in acid? Explain
Compare and contrast a voltaic cell and an electrolytic cell with respect to each of the following:
(a) Sign of the free energy change
(b) Nature of the half-reaction at the anode
(c) Nature of the half-reaction at the cathode
(d) Charge on the electrode labelled 鈥渁node鈥�
(e) Electrode from which electrons leave the cell
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