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Chapter 21: Q21.22 P (page 973)

Consider the following general voltaic cell:

Identify the (a) anode, (b) cathode, (c) salt bridge, (d) electrode at which leave the cell, (e) electrode with a positive charge, and electrode that gains mass as the cell operates (assuming that a metal plates out).

Short Answer

Expert verified

(a) A

(b) E

(c) C

(d) A

(e) E

(f) E

Step by step solution

01

Definition of Chemical Change and Electrical Work 

Electrochemistry is a discipline of physical chemistry concerned with the relationship between electrical potential as a quantifiable and quantitative phenomenon and recognisable chemical change, with electrical potential as an outcome of a specific chemical change or vice versa.

02

Identify the following general voltaic cell

A voltaic cell is an electrochemical cell that generates electricity by a spontaneous redox reaction.

We can deduce the following from the diagram:

(a) Anode:A

(b) Cathode:E

(c) Salt bridge:C

(d) Electrode where leaves the cell:A

(e) Positively charged electrode:E

(f) An electrode that accumulates mass while the cell works: E

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Most popular questions from this chapter

What are E∘cell and△G∘ of a redox reaction at250Cfor which n=1 andK=5.0×104.

Which statements are true? Correct any that are false.

(a) In a voltaic cell, the anode is negative relative to the cathode.

(b) Oxidation occurs at the anode of a voltaic or electrolytic cell.

(c) Electrons flow into the cathode of an electrolytic cell.

(d) In a voltaic cell, the surroundings do work on the system.

(e) A metal that plates out of an electrolytic cell appears on the cathode.

(f) The cell electrolyte provides a solution of mobile electrons.

A chemist designs an ion-specific probe for measuring [ Ag+] 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 ( Hg2Cl2)] in a saturated KCl solution. The measuredEcell is 0.060V. (a) Given the following standard half-reactions, calculate [Ag+ ].

Calomel:Hg2Cl2(s) + 2e-→2Hg + 2Cl-Eo= 0.24 V

Silver:Ag+(aq) +e-→Ag(s)Eo= 0.80 V

(Hint: Assume [ Cl-] is so high that it is essentially constant.) (b) A mining engineer wants an ore sample analyzed with theAg+ - selective probe. After pre-treating the ore sample, the chemist measures the cell voltage as V. What is [ Ag+]?

A Voltaic cell consists of a metal A/A+ electrode and a metal B/B+ electrode, with theA/A+ electrode negative. The initial[A+]/[B+] is such thatrole="math" localid="1659592400010" Ecell >role="math" localid="1659592428249" Ecello

(a) How dorole="math" localid="1659592855546" [A+] and [B+]change as the cell operates?

(b) How doesrole="math" localid="1659592922361" Ecell change as the cell operates?

(c) What is role="math" localid="1659592941387" [A+]/[B+] whenEcell =role="math" localid="1659592990948" Ecello ? Explain.

(d) Is it possible forrole="math" localid="1659593025964" Ecell to be less than Ecello? Explain

In an aqueous electrolytic cell, nitrate ions never react at the anode, but nitrite ions do. Explain.
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