Corrosion of silver in fused nitrates: Applications of E/pO2− diagrams

Conte, A.; Ingram, Malcolm D.

doi:10.1016/0013-4686(68)80138-0

Cited by 20 publications

(12 citation statements)

References 6 publications

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“…[26][27][28][29][30] Most of the studies on LSM indicate that LSM does not react with the Ba-containing materials. [31][32][33] However, considering the polarization effect, particularly the strong corrosivity of nitrate under polarization and heating, [34][35][36] the reaction between the electrode materials and the Ba compounds is possible. Traulsen et al 12 reported a distinct change in the microstructure on the LSM/CGO cell stacks inltrated with BaO aer the electrochemical test and attributed it to the reaction between BaO and LSM/CGO under the test conditions.…”

Section: Degradation Related To the Microstructure Changementioning

confidence: 99%

Electrochemical NOx reduction on an LSM/CGO symmetric cell modified by NOx adsorbents

Shao

2013

J. Mater. Chem. A

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Section: Degradation Related To the Microstructure Changementioning

confidence: 99%

Electrochemical NOx reduction on an LSM/CGO symmetric cell modified by NOx adsorbents

Shao

2013

J. Mater. Chem. A

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“…This was Paper 499 presented at the Las Vegas, NV, Meeting of the Society, October [13][14][15][16][17][18] 1985. This was Paper 499 presented at the Las Vegas, NV, Meeting of the Society, October [13][14][15][16][17][18] 1985.…”

Section: Acknowledgmentsmentioning

confidence: 99%

“…This sort of presentation has already been used to study the thermodynamic properties of several metals in molten nitrate and molten nitrite salts (12)(13)(14). This sort of presentation has already been used to study the thermodynamic properties of several metals in molten nitrate and molten nitrite salts (12)(13)(14).…”

mentioning

confidence: 99%

Thermodynamic Study of Corrosion of Iron in NaNO3 ‐ NaNO2 Mixtures

Picard

Lefèbvre

Trémillon

1987

J. Electrochem. Soc.

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phology is consistent with the relatively rapid doping kinetics and the associated electrochromism of PITN. Since the characteristic switching time is expected to vary as the square of the radius of the microfibrils (see Eq.[4]), it should be possible to improve the switching speed by decreasing the size of the subunits. Our conclusion is that the detailed morphology plays a critical role in determining the electrochromic switching; by controlling the morphology so as to minimize the diffusion distance in conductive polymers, it should be possible to achieve sufficient speed to be of interest for a variety of technological applications. Ma'ABSTRACT The influence of oxoacidity on the corrosion of iron in molten sodium nitrate-nitrite mixtures has been demonstrated by means of potential-pO 2-diagram. Oxoacidobasic titrations of iron(III) have been carried out by means of potentiometric measurements with an yttria-stabilized zirconia membrane electrode, indicator of pO 2-. They have shown the formation of three different species of iron(III) and have allowed the determination of experimental oxoacidity constants in the temperature range from 693 to 773 K. These results and the thermochemical data of the literature have been used to establish the potential-pO 2-diagram relative to iron. This diagram permits one to forecast that three different compounds may be formed, according to the pO 2-, when iron is in contact with the salt: Fe2054-or Na4Fe2Os(s) in strongly basic media, FeO2-or NaFeO~(s) in moderately basic media, Fe203(s) in acidic media. A good correlation exists between our predictions and the corrosion tests reported in the literature. ) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 132.174.254.155 Downloaded on 2015-04-05 to IP Vol. I34, No. 1 ) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 132.174.254.155 Downloaded on 2015-04-05 to IP ) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 132.174.254.155 Downloaded on 2015-04-05 to IP ABSTRACTIn this investigation, the effect of alloying on catalysis, especially with respect to oxygen and the ORR, was examined. A series of PtCr alloys allowed four major aspects of alloying to be investigated: (i) effect of decreasing lattice parameter with increasing Cr content in the Pt terminal solid solution, (it) effect of an order/disorder transition, (iii) difference between intermetallic and solid solution structures, and (iv) effect of dendritic segregation. Results indicated that contrary

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“…Although perceptible decomposition of Ag~O into its elements occurs above 160~ (20), the kinetics of this reaction are rather slow, as found in classical studies many years ago by Lewis and others (32)(33)(34). [7] or from the reaction of Ag~O with nitrite ions (21) Ag20 + NO2---> 2Ag + NO3- [8] Possible corrosion reactions of silver and their estimated E ~ values at 350~ in molten LiNO3 include Ag(~ + NO..,~g) + 1/2 O2(g) ~ AgNO3(,) (E ~ = 0.13V) [9] 2Ag(s) + LiNO3(,) ~ Ag~O(s) + LiNO~(,) (E ~ = -0.28V) [10] 2Ag(~) + 3LiNO3(l) '+ H20(I, ~ 2AgNO~I) + LiNO~(I) + 2LiOH(~) (E ~ = -0.63V) [11] 2Ag(sl + 2LiNO3,j) + 1/20=,(g) ~ 2AgNO3(1) + Li~O(~) (E ~ -0.78V) [12] The latter three reactions are possible only when the reaction products are present at low activities. This precipitate remains unchanged at temperatures up to 350~ suggesting that the rate of decomposition of Ag~O is quite slow in molten nitrates.…”

Section: Lino~ At 350~mentioning

confidence: 99%

“…Problems encountered in cell EMF measurements have suggested the corrosion of silver electrodes in fused nitrates (23,24). Thermodynamic calculations of potential vs. pO 2-diagrams for silver in fused nitrates predict that silver is less stable in molten LiNO3 than in the NaNO3-KNO3 eutectic melt (21). Thermodynamic calculations of potential vs. pO 2-diagrams for silver in fused nitrates predict that silver is less stable in molten LiNO3 than in the NaNO3-KNO3 eutectic melt (21).…”

mentioning

confidence: 99%

Reactions Involving Silver Ions and Silver Metal in Molten Nitrates

Miles¹,

McManis²,

Fletcher³

1984

J. Electrochem. Soc.

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Regarding quarternary systems, the introduction of the composition parameters y, t, and S serves in the planning of experiments and in reducing the large number of compositions to be studied in order to characterize a quarternary system adequately.Also, the use of these composition parameters makes it possible to plot thermodynamic data along well-defined composition paths and to identify the effects of competing interactions on a charge asymmetric cation. For example, the complexing effects of CsC1 or KC1 on MnCI~ become evident as the quarternary solutions become richer in CsC1, or in KC1, respectively.The successful application of Eq.[15], [16], and [17] to such nonideal charge asymmetric fused-salt solutions indicates that in quarternary, and possibly even in higher order systems, reactions within the binary solutions account for most of the internal reactivity which is responsible for deviations from ideality. Thus, the formation of a higher order system represents mixing of such prereacted binary systems and the properties of the multicomponent system should be predictable.However, it should be noted that Eq.[15], [16], and [17] are only applicable to the "acid," or higher valence, component of a charge asymmetric fused-salt mixture. ABSTRACTThe electrochemical reduction of molten LiNO3 on platinum or nickel electrodes produces insoluble LifO that passivates the cathode at high current densities. The presence of small amounts of silver ions prevents this passivation by undergoing reduction to silver metal in the form of dendritic deposits that increase the effective area of the electrode. The deposited silver is unstable in molten LiNO3 and reacts with the melt to regenerate silver ions. Corrosion studies of silver coupons gave a weight loss rate of 280 ~g h-lcm -2 in molten LiNO3 at 350~ but of only 5 ~g h-lcm -2 in KNO~ at 375~ The presence of water in the LiNO3 melt increases the corrosion rate of silver. Additions of Li20, LiNO2, LiC1, or AgNO3 to molten LiNO3 significantly decreases the corrosion rate. The addition of oxide ions to a AgNO~ containing melt produces a dark precipitate of Ag20 in NaNO~ or KNO3, but not in LiNO3. The decomposition reaction of Ag20 into its elements is kinetically slow in molten nitrates with a rate similar to that observed in air.) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 169.230.243.252 ABSTRACTThe photoelectrochemical properties of n-SiC were studied in aqueous electrolytes. The onset potential of the anodic photocurrent in steady state was found to be about 1V more anodic than that of the photocurrent measured by the lock-in method (-2V vs. SCE). This discrepancy was ascribed to the presence of transient photocurrent observed in the potential range between -1.9 and +0.6V vs. SCE. Possible mechanisms of the transient photoresponse were exam-

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Corrosion of silver in fused nitrates: Applications of E/pO2− diagrams

Cited by 20 publications

References 6 publications

Electrochemical NOx reduction on an LSM/CGO symmetric cell modified by NOx adsorbents

Electrochemical NOx reduction on an LSM/CGO symmetric cell modified by NOx adsorbents

Thermodynamic Study of Corrosion of Iron in NaNO3 ‐ NaNO2 Mixtures

Reactions Involving Silver Ions and Silver Metal in Molten Nitrates

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