Abstract
As was shown in Chap. 4, the behaviour of real electrochemical systems on long timescales cannot often be predicted from short-term observations. In terms of the approach considered in 1.6, this happens because of the onset of positive feedbacks destabilising the stationary state of the system. Several possible reasons exist for this event to take place. Among them, most significant, however very rarely considered, is the coupling between the electrochemical processes at separate electrodes. To understand how it works, we shall first consider the process of electrochemical decomposition of an electrolyte with mixed ion–electron conductivity.
Irreversible phenomena are much more stubborn. However even they tend to enter the general order.
H. Poincarè
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Notes
- 1.
Such estimation is not much reliable due to the lack of experimental data on the viscosity and density of the melts at different temperatures. However, it is in agreement with the value (2÷3)⋅10–2 cm which was obtained by direct optical measurements [15] for conditions of free convection in the chloride melts.
References
Velikanov AA (1971) Electrochemical investigation of chalcogenide melts. Dr of Sciences Thesis, Institute of General and Inorganic Chemistry, Kiev
Velikanov AA (1974) Electronic-ionic conductivity of non-metal melts. In: Ionic melts, vol 2. Naukova Dumka, Kiev, p 146–154
Velikanov AA (1974) Electrochemistry and melts. Nauka, Moscow
Belous AN (1978) Studies on the electrode processes at the electrodeposition of thallium, lead and tin from sulfide and sulfide–chloride melts. PhD (Kandidate) Thesis, Institute of General and Inorganic Chemistry, Kiev
Zagorovskii GM (1979) Electrochemical investigations of molten systems based on antimony sulfide. PhD (Kandidate) Thesis, Institute of General and Inorganic Chemistry, Kiev
Vlasenko GG (1979) Electrochemical investigations of sulfide–chloride melts. PhD (Kandidate) Thesis, Institute of General and Inorganic Chemistry, Kiev
Lysin VI (1985) Studies on the nature of conductivity and electrochemical polarization in Chalcogenide–halogenide melts. PhD (Kandidate) Thesis, Institute of General and Inorganic Chemistry, Kiev
Mon’ko AP, Andriiko AA (1999) Ukrainian Chem J 65:111–118
Andriiko AA, Mon’ko AP, Lysin VI, Tkalenko AD, Panov EV (1999) Ukrainian Chem J 65: 108–114
Andriiko AA, Panov EV, Mon’ko AP, Lysin VI (2002) Visnyk Lvivskoho Universytetu (Bulletin of Lviv University). Chemistry 42:109–113
Wagner C (1956) Z Elektrochem 60:4–12
Yokota I (1953) J Phys Soc Jpn 8:595–598
Hebb MH (1952) J Chem Phys 20:185–189
Zinchenko VF, Lisin VI, Il’chenko AI (1991) Ukrainian Chem J 57:389–393
Polyakov PV, Isaeva LI, Anokhina VS (1975) Izvestiya VUZov. Tsvetnye metally 6:73–76
Shevchuk PP, Velikanov AA, Malinovskii VV, Ivanova EI (1973) Elektrokhimiya 9: 1984–1988
Izgaryshev NA, Grigor’ev NK (1936) Zhurnal Obschei Khimii (Russ J Gen Chem) 6: 1676–1683
Andriiko AA, Panov EV, Mon’ko AP (1998) J Solid State Electrochem 2:198–203
Migulin VV (1986) Fundamentals of oscillation theory. Nauka, Moscow (in Russian)
Bogoliubov NN, Mitropol’skiy YA (1974) Asymptotic methods in theory of non-linear oscillations. Nauka, Moscow (in Russian)
Sal’nikov IE (1949) Russ J Phys Chem 23:258–270
Vol’ter BV, Sal’nikov IE (1981) Stability of operation regimes of chemical reactors. Khimija, Moscow (in Russian)
Engelgardt GR, Dikusar AI (1986) J Electroanal Chem 207:1–8
Godshall NA, Driscoll JR (1984) J Electroanal Chem 131:2291–2297
Kuz’minskii YV, Andriiko AA, Nyrkova LI (1993) J Power Sources 46:29–38
Szpak S, Gabriel CJ, Driscoll JR (1987) Electrochim Acta 32:239–246
Andriiko AA, Kuz’minskii YV (1993) J Power Sources 45:303–310
Semenov NN (1986) Chain reactions, Part I. Nauka, Moscow (in Russian)
Tchebotin VN (1982) Physical chemistry of solids. Khimija, Moscow (in Russian)
Kamarchik P, Margrave JL (1977) J Therm Anal Calorim 11:259–264
Reissig P, Sansone H, Conti P (1974) Qualitative theory of nonlinear differential equations. Nauka, Moscow
Andriiko AA (1990) Rasplavy (Russian Journal “Melts”) 1:65–73
Andriiko AA, Delimarskii YK, Tchernov RV (1984) Ukrainian Chem J 50:1174–1179
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Appendices
Appendix A. Derivation of the Differential Equations (5.11) and (5.12)
Because of the mixed conductivity of the anodic film, the Faradaic process at the anode splits into two, i.e. at the inner junction (metal/film) and the outer one (film/electrolyte).
Let us denote the ionic current part as α. Then, at current I and in a lime interval of dt the quantity of deposit
is formed at the inner junction.
At the outer junction, (1 – α)Idt Coulombs of electricity are consumed at the same time to oxidise the portion of the film substance dμ ext, and the portion of the intermediate transferred from the bulk by the flux J c is
To determine the flux, Nernst model of stationary diffusion with linear distribution of the concentration across the layers of the constant thickness is used, and the concentration of the intermediate is assumed to be zero, i.e. the anode discharge proceeds at limit current condition. Then
The differential equation (Eq. 5.11) is obtained by combination of the equation for the material balance of the film substance
Equation (5.12) can be obtained from the balance of the intermediate in the electrolyte, which is supported by the cathodic flux J c to the bulk and the anodic flux J a from the bulk
Apart from the above-mentioned Nernst diffusion, the following assumptions and approximations were made in the derivation of Eq. (5.12).
Intervalent equilibrium between polyvalent species at the cathode surface is assumed to establish. A convenient notation of this equilibrium, according Chap. 2, is
where the symbols E(0), E(i), and E(N) correspond to polyvalent metal compounds, oxidation numbers being zero, i, and N, respectively.
The activity of E(0) is regarded to be 1 (solid pure metal). Further, the concentration C N of the high-valence compound E(N) at the surface of the cathode and in the bulk is assumed to be equal. This is acceptable for not very dilute solutions. We can now express the cathodic surface concentration of the intermediate by
Further, the charge balance equation in the form
is used, where C o is the total initial concentration of the electrolyte. This means that the electrolyte at the initial time condition contains only the high-valence compound E(N) with a concentration of C o, and no additions of salts to the melt during the process are made.
Now the cathodic concentration C i,cath required for the determination of the flux
can be obtained by determining C N from Eq. (8a) and substituting it into Eq. (7a). The obtained power function may be expanded into a series and, after neglecting the second and higher order members, may be written in the form
This linearising simplification is sufficiently correct when the condition is fulfilled
Finally, Eq. (5.12) is obtained by substitution of Eqs. (3a), (9a), and (10a) into Eq. (5a).
Appendix B. Approximate Solution of the Non-linear Second-Order Differential Equation by Small-Parameter (Krylov–BogoIiubov) Method [20]
If the non-linear term of the differential equation may be thought of as a small disturbance, the above-mentioned method can then be applied to derive an approximate solution. Equation (5.35) is presented as follows:
where
and non-linear function
The solution is sought in the form
by a common technique described elsewhere [19, 20].
Finally, the approximate periodic solution of the limit cycle type is obtained in the form
where the dimensionless frequency w is approximately equal to \( \sqrt{{a-\gamma }} \). The dimensionless period \( T=2\pi /w \) of the oscillation, then, is equal to \( {{{2\pi }} \left/ {{\sqrt{{a-\gamma }}}} \right.} \). Therefore, the formula of Eq. (5.36) for the real timescale period is accurate to a constant coefficient. This coefficient is of the order 1 and should increase as the current I and concentration C 0 increase. This is hard to verify experimentally because of the very long duration of the tests.
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Andriiko, A.A., Andriyko, Y.O., Nauer, G.E. (2013). Dynamics of a Non-equilibrium Electrochemical System. In: Many-electron Electrochemical Processes. Monographs in Electrochemistry. Springer, Berlin, Heidelberg. https://doi.org/10.1007/978-3-642-35770-1_5
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