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In electrochemical kinetics, the concept of the electrode potential is employed in a more general sense, and designates the electrical potential difference between two identical metal leads, the first of which is connected to the electrode under study (test, working or indicator electrode) and the second to the reference electrode which is in a currentless state Electric current flows, of course, between the test electrode and the third, auxiliary, electrode The electric potential difference between these two electrodes includes the ohmic potential difference as discussed in Section 552 If current passes through an electrolytic cell, then the potential of each of the electrodes attains a value different from the equilibrium value that the electrode should have in the same system in the absence of current flow This phenomenon is termed electrode polarization.

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*A:NS074662074# configure system name Dev4-CE2 *A:Dev4-CE2# configure card 1 card-type iom-20g-b *A:Dev4-CE2# configure card 1 mda 1 mda-type m10-1gb-sfp-b *A:Dev4-CE2# configure port 1/1/1 no shutdown *A:Dev4-CE2# configure router *A:Dev4-CE2>config>router# interface system *A:Dev4-CE2>config>router>if# address 150.10.0.2/32 *A:Dev4-CE2>config>router>if# exit *A:Dev4-CE2>config>router# interface toVPLS *A:Dev4-CE2>config>router>if$ address 192.168.0.4/24 *A:Dev4-CE2>config>router>if$ port 1/1/1 *A:Dev4-CE2>config>router>if$ exit *A:Dev4-CE2>config>router#

When a single electrode reaction occurs at a given current density at the electrode, then the degree of polarization can be defined in terms of the overpotential The overpotential r\ is equal to the electrode potential E under the given conditions minus the equilibrium electrode potential corresponding to the considered electrode reaction Ee: rj = E-Ec (5111).

3. (Optional) On Device4, create OSPF area 0. Add the system interface and interface connecting to the PE2.

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However, the value of the equilibrium electrode potential is often not well defined (e.g. when the electrode reaction produces an intermediate that undergoes a subsequent chemical reaction yielding one or more final products). Often, an equilibrium potential is not established at all, so that the calculated equilibrium values must often be used. It should also be recalled that, for many electrodes in various solutions, the open circuit electrode potential, i.e. the electrode potential in the absence of current flow, is not the thermodynamic equilibrium but rather a mixed potential, discussed in Section 5.8.4. Polarization is produced by the slow rate of at least one of the partial processes in the overall electrode process. If this rate-controlling step is a transport process, then concentration polarization is involved; if it is the charge transfer reaction, then it is termed charge transfer polarization, etc. Electrode processes are often classified on this basis.

*A:Dev4-CE2>config>router# ospf *A:Dev4-CE2>config>router>ospf$ area 0 *A:Dev4-CE2>config>router>ospf>area$ interface system *A:Dev4-CE2>config>router>ospf>area>if$ exit *A:Dev4-CE2>config>router>ospf>area# interface toVPLS *A:Dev4-CE2>config>router>ospf>area>if$ exit *A:Dev4-CE2>config>router>ospf>area# exit *A:Dev4-CE2>config>router>ospf# exit *A:Dev4-CE2>config>router#

Albery, W. J., Electrode Kinetics, Clarendon Press, Oxford, 1975. Bamford, C. H., and R. G. Compton (Eds), Electrode Kinetics Principles and Methodology, Elsevier, Amsterdam, 1986. Compton, R. G. (Ed.), Electrode Kinetics, Elsevier, Amsterdam, 1988. Damaskin, B. B., and O. A. Petrii, Introduction into Electrochemical Kinetics (in Russian), Vysshaya shkola, Moscow, 1975. Gerischer, H., Semiconductor electrode reactions, AE, 1, 31 (1961). Gerischer, H., Elektrodenreaktionen mit angeregten elektronischen Zustanden, Ber. Bunsenges., 77, 771 (1973). Hush, N. S. (Ed.), Reactions of Molecules at Electrodes, Wiley-Interscience, New York, 1970. Kinetics and Mechanisms of Electrode Processes, CTE, 7 (1983). Krishtalik, L. I., Charge transfer in Chemical and Electrochemical Processes, Plenum Press, New York, 1986. Morrison, S. R., Electrochemistry at Semiconductor and Oxidized Metal Electrodes, Plenum Press, New York, 1980. Myamlin, V. A., and Yu. V. Pleskov, Electrochemistry of Semiconductors, Plenum Press, New York, 1967. Southampton Electrochemistry Group (R. Greef, R. Peat, L. M. Peter, D. Pletcher, and J. Robinson), Instrumental Methods in Electrochemistry, Ellis Horwood, Chichester, 1985. Vetter, K. J., Electrochemical Kinetics, Academic Press, New York, 1967. Vielstich, W., and W. Schmickler, Elektrochemie II. Kinetik elektrochemischer Systeme, Steinkopf, Darmstadt, 1976.

4. Confirm basic connectivity between the CE devices by pinging the interfaces on the 192.168.0.0/24 subnet. If there is no response, verify the previous configuration steps and correct as necessary. Pay particular attention to the configuration of addresses on CE1 and Device4.

5.2 5.2.1

*A:CE1# ping 192.168.0.4 PING 192.168.0.4 56 data bytes 64 bytes from 192.168.0.4: icmp_seq=1 64 bytes from 192.168.0.4: icmp_seq=2 64 bytes from 192.168.0.4: icmp_seq=3 64 bytes from 192.168.0.4: icmp_seq=4