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Chapter 21: Q21.93P (page 922)
Identify those elements that can be prepared by electrolysis of their aqueous salts: copper, barium, aluminum, bromine.
Elements that can be prepared by electrolysis of their aqueous salt: Bromine and copper.
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A chemist designs an ion-specific probe for measuring [ ] in an NaCl solution saturated with AgCl. One half-cell has an Ag-wire electrode immersed in the unknown AgCl saturated NaCl solution. It is connected through a salt bridge to the other half-cell, which has a calomel reference electrode [a platinum wire immersed in a paste of mercury and calomel ( )] in a saturated KCl solution. The measured is V. (a) Given the following standard half-reactions, calculate [ ].
Calomel:
Silver:
(Hint: Assume [ ] is so high that it is essentially constant.) (b) A mining engineer wants an ore sample analyzed with the - selective probe. After pre-treating the ore sample, the chemist measures the cell voltage as V. What is [ ]?
A voltaic cell is constructed with a half-cell and an half-cell. The nickel electrode is negative.
(a) Write balanced half-reactions and the overall reaction.
(b) Diagram the cell, labeling electrodes with their charges and showing the directions of electron flow in the circuit and of cation and anion flow in the salt bridge
Consider the following balanced redox reaction:
(a) Which species is being oxidized?
(b) Which species is being reduced?
(c) Which species is the oxidizing agent?
(d) Which species is the reducing agent?
(e) From which species to which does electron transfer occur?
(f) Write the balanced molecular equation, with as the spectator ions.
A voltaic cell using Cu/ and Sn/ half-cells is set up at standard conditions, and each compartment has a volume of345mL. The cell delivers 0.17 A for h. (a) How many grams of Cu(s) are deposited? (b) What is the [ ] remaining?
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 “anode”
(e) Electrode from which electrons leave the cell
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