209:
305:
In 1953 in
Stockholm IUPAC recognized that either of the conventions is permissible; however, it unanimously recommended that only the magnitude expressed according to the convention (2) be called "the electrode potential". To avoid possible ambiguities, the electrode potential thus defined can also
517:
This follows from the IUPAC definition of the electric potential difference of a galvanic cell, according to which the electric potential difference of a cell is the difference of the potentials of the electrodes on the right and the left of the galvanic cell. When
512:
446:
149:
367:. Proponents of the convention (2) argue that all reported electrode potentials should be consistent with the electrostatic sign of the relative potential difference.
158:
at the working electrode ("reversible potential"), or a potential with a non-zero net reaction on the working electrode but zero net current ("corrosion potential", "
226:
92:
In an electrochemical cell, the cathode and the anode have certain electrode potentials independently and the difference between them is the cell potential:
458:
17:
395:
669:
613:
609:
384:
642:
C.A. Hamel, "The
Encyclopedia of Electrochemistry", Reinhold Publishing Corporation, New York-Chapman & Hall Ltd., London, 1964, p. 429–431.
98:
310:. In both conventions, the standard hydrogen electrode is defined to have a potential of 0 V. Both conventions also agree on the sign of
196:
involves this reference electrode with hydrogen ion in an ideal solution having is "zero potential at all temperatures" equivalently to
181:
The value of the electrode potential under non-equilibrium depends on the nature and composition of the contacting phases, and on the
651:
P. van
Rysselberghe, "Bericht der Kommission für electrochemische Nomenklatur und Definitionen", Z. Electrochem., 58 (1954), 530–535.
581:
61:
The electrode potential has its origin in the potential difference developed at the interface between the electrode and the
712:
363:
switches sign when a reaction is written in reverse, so too, proponents of the convention (1) argue, should the sign of
246:
in the electrolyte, e.g., by positioning the reference electrode near the surface of the working electrode (e.g., see
389:
Potential of a cell assembled of two electrodes can be determined from the two individual electrode potentials using
197:
85:
due to the transfer of charged species across the interface, specific adsorption of ions at the interface, and
317:
The main difference between the two conventions is that upon reversing the direction of a half-cell reaction
660:
Anson, Fred C. "Common sources of confusion; Electrode Sign
Conventions," J. Chem. Educ., 1959, 36, p. 394.
576:
545:
171:
380:
58:. It may also be defined as the potential difference between the charged metallic rods and salt solution.
255:
193:
51:
186:
707:
155:
283:
182:
325:
also switches, whereas in the convention (2) it does not. The logic behind switching the sign of
586:
356:. It is assumed that the half-reaction is balanced by the appropriate SHE half-reaction. Since
251:
159:
528:
is positive, then positive electrical charge flows through the cell from the left electrode (
78:
290:
279:
376:
8:
262:
connected to the working electrode and the negative terminal to the reference electrode.
232:
50:
and another electrode to be characterized. By convention, the reference electrode is the
216:
The measurement is generally conducted using a three-electrode setup (see the drawing):
550:
163:
555:
385:
Electrolytic cell § Anode and cathode definitions depend on charge and discharge
330:
220:
679:
623:
686:
674:
627:
618:
507:{\displaystyle \Delta V_{\text{cell}}=E_{\text{red,cathode}}+E_{\text{oxy,anode}}.}
353:
247:
31:
441:{\displaystyle \Delta V_{\text{cell}}=E_{\text{red,cathode}}-E_{\text{red,anode}}}
239:
In case of non-zero net current on the electrode, it is essential to minimize the
192:
An operational assumption for determinations of the electrode potentials with the
591:
560:
294:
174:
for a given electroactive species by extrapolation of the measured values to the
162:"), or a potential with a non-zero net current on the working electrode (like in
270:
Historically, two conventions for sign for the electrode potential have formed:
275:
175:
258:. The potential measurements are performed with the positive terminal of the
701:
678:, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "
622:, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "
565:
370:
86:
43:
690:
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82:
65:. It is common, for instance, to speak of the electrode potential of the
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144:{\displaystyle E_{\text{cell}}=E_{\text{cathode}}-E_{\text{anode}}.}
570:
533:
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89:/orientation of polar molecules, including those of the solvent.
39:
529:
55:
314:
for a half-cell reaction when it is written as a reduction.
212:
Three-electrode setup for measurement of electrode potential
170:). Reversible potentials can be sometimes converted to the
371:
Potential difference of a cell assembled of two electrodes
329:
is to maintain the correct sign relationship with the
461:
398:
101:
27:
Electromotive force of a cell built of two electrodes
200:
of hydrogen ion is also "zero at all temperatures".
506:
440:
143:
54:(SHE). It is defined to have a potential of zero
699:
235:(standard hydrogen electrode or an equivalent).
321:, according to the convention (1) the sign of
154:The electrode potential may be either that at
72:
381:Electrochemical cell § Cell potential
348:is the number of electrons involved and
301:" (sometimes referred to as "European").
286:" (sometimes referred to as "American"),
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14:
700:
582:Table of standard electrode potentials
308:Gibbs–Stockholm electrode potential
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77:Electrode potential appears at the
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18:Electrochemical corrosion potential
680:electric potential difference, ΔV
675:Compendium of Chemical Terminology
636:
619:Compendium of Chemical Terminology
462:
399:
25:
724:
377:Galvanic cell § Cell voltage
46:built from a standard reference
183:kinetics of electrode reactions
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654:
645:
603:
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198:standard enthalpy of formation
13:
1:
597:
577:Standard electrode potential
546:Absolute electrode potential
172:standard electrode potential
7:
539:
194:standard hydrogen electrode
52:standard hydrogen electrode
10:
729:
713:Electrochemical potentials
532:) to the right electrode (
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81:between an electrode and
73:Origin and interpretation
691:10.1351/goldbook.E01934
632:10.1351/goldbook.E01956
624:electrode potential, E
587:Thermodynamic activity
508:
442:
252:supporting electrolyte
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187:Butler–Volmer equation
185:at the interface (see
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509:
448:however , it depends.
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254:of sufficiently high
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571:Potential difference
459:
396:
99:
233:reference electrode
87:specific adsorption
36:electrode potential
682:of a galvanic cell
551:Electric potential
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452:or, equivalently,
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306:be referred to as
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164:galvanic corrosion
141:
556:Galvani potential
498:
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333:change, given by
331:Gibbs free energy
250:), or by using a
227:counter electrode
221:working electrode
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16:(Redirected from
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708:Electrochemistry
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561:Nernst equation
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176:standard state
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69:redox couple.
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566:Overpotential
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44:galvanic cell
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289:convention "
274:convention "
269:
260:electrometer
256:conductivity
238:
215:
191:
180:
153:
91:
76:
60:
35:
29:
484:red,cathode
421:red,cathode
204:Measurement
168:voltammetry
156:equilibrium
83:electrolyte
63:electrolyte
702:Categories
598:References
375:See also:
319:as written
573:(voltage)
497:oxy,anode
463:Δ
434:red,anode
426:−
400:Δ
299:Stockholm
126:−
79:interface
48:electrode
540:See also
534:cathode
352:is the
295:Ostwald
284:Latimer
244:IR-drop
121:cathode
40:voltage
38:is the
383:, and
344:where
276:Nernst
670:IUPAC
614:IUPAC
610:IUPAC
530:anode
291:Gibbs
280:Lewis
241:ohmic
134:anode
56:volts
42:of a
525:cell
471:cell
408:cell
108:cell
687:doi
685:".
628:doi
626:".
536:).
341:nFE
339:= –
189:).
166:or
67:M/M
30:In
704::
672:,
616:,
612:,
379:,
178:.
34:,
689::
630::
522:V
520:Δ
502:.
493:E
489:+
480:E
476:=
467:V
430:E
417:E
413:=
404:V
365:E
360:G
358:Δ
350:F
346:n
337:G
335:Δ
327:E
323:E
312:E
297:–
293:–
282:–
278:–
229:,
223:,
139:.
130:E
117:E
113:=
104:E
20:)
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