Abusive testing of large Li/SOCl2 cells

Marinčić, N.; Goebel, F.

doi:10.1016/0378-7753(80)80096-6

Cited by 9 publications

(2 citation statements)

References 4 publications

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“…Soon after the discovery of the lithium/thionyl chloride electrochemical cell, optimization studies led to the development of storable, high performance cells suitable for a variety of applications (1,2). It was realized, however, that cells with sulfuryl chloride (SO2,C12) rather than thionyl chloride (SOC12) as the oxyhalide might offer some advantages.…”

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confidence: 99%

The Lithium/Sulfuryl Chloride Electrochemical Cell

Klinedinst¹

1984

J. Electrochem. Soc.

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The development of a practical sulfuryl chloride‐based lithium/oxyhalide cell technology has been delayed by anode corrosion and cathode polarization problems encountered when the standard oxyhalide cell electrolyte and cathode formulations are used. The anode stability problem can be significantly alleviated by the use of a reverse polarity cell design, the substitution of Li2B10Cl10 for LiAlCl4 as the electrolyte salt, and the addition of a suitable cosolvent ( SO2 or SOCl2 ). Further, at least under ambient temperature storage and discharge conditions, anode passivation is completely absent with hermetically sealed normalLi/SO2Cl2 cells of this type. Cathode polarization can be reduced most effectively by the use of a supported platinum cathode material. This cathode material also results in substantially increased discharge capacities, although the overall reaction stoichiometry is unaffected by the catalyst. Finally, SO2Cl2 thermal decomposition measurements indicate that, as the temperature of the SO2Cl2 electrolyte in a hermetic cell is increased from 25° to 80°C, the pressure differential across‐the cell case will rise to about 3.5 atm. Then, as the temperature is decreased to a lower value, the pressure differential will also decrease to the equilibrium value characteristic of that lower temperature, indicating a thermally stable, reversible system.

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confidence: 99%

The Lithium/Sulfuryl Chloride Electrochemical Cell

Klinedinst¹

1984

J. Electrochem. Soc.

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“…Solutions saturated with sulfur and sulfur dioxide, with and without LiAICI4, with and without fresh or used cathode material, failed to produce hysteresis similar to that seen for the used electrolyte, even when the fresh mixtures were recycled to 100~ Reactions [10], [11], or [12] could therefore not have occurred under these conditions. Figure 14 shows the result when used electrolyte was so cycled.…”

Section: Vt : E ~-T (Oe/ot) : --(~H/nf) : 334v [8]mentioning

confidence: 94%

Discharge Reaction Mechanisms in Li / SOCl2 Cells

Schlaikjer¹,

Goebel²,

Marinčić³

1979

J. Electrochem. Soc.

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The processes taking place during the discharge of Li/SOC12/C cells were studied. Test vehicles included wound D, bobbin configuration 2D cells, and 2000 A-hr prismatic cells. Dried cathodes taken from 2D cells, discharged at 150 mA were analyzed quantitatively for lithium-sulfur oxyaeid salts. Little or no such salt was found for cells discharged at ambient temperature. Measurements of the open-circuit voltage of this system as a function of temperature showed essentially linear dependence with positive slope between ~-72 ~ and --20~ but the voltage fell more steeply as the temperature approached --60~Appearance of a nonvolatile reducing species occurred in the cathodes of cells discharged at --20~ which were not present in cathodes from cells discharged at higher temperature. Controlled potential electrolysis of supporting electrolytes containing limited amounts of SOCI.~ were carried out between 0 ~ and 25~ The electrical equivalent of thionyl chloride was found to be between 1.5 and 2.0 F/mole. The 200,0 A-hr cells were used to measure dissolved SO2 and SO2 escaping at atmospheric pressure and ambient temperature from anode-limited and cathode-limited cells. The amount of SO2 produced was found to be only a fraction of that predicted by 4Li ~-2SOCls -+ S § SO2 + 4LiC1 until near the end of discharge. The total amount of SOs produced by the end of discharge was not more than predicted by this reaction. Vented, anode-limited cells did not release SO2 while cathode-limited cells did. Temperature cycling of electrolyte taken from cells immediately after discharge was carried out in a sealed vessel. Pressure hysteresis occurred, which could not be duplicated with simulated used electrolyte made with S, SOs, SOC12, LiA1C14, and cathode material. At --20~ and below, the discharge reaction 8Li + 3SOCls-~ 2S ~-Li2SO8 ~-6LiC1 may be significant, while at temperatures higher than this, the reaction 2nLi + nSOC12-~ 2nLiC1 + (SO), may predominate, where the (SO)n remains in solution. Slow decomposition according to (SO)h-> (n/2)S + (n/2)SOz may subsequently take place.

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Lithium Batteries with Liquid Depolarizers

Marinčić

1983

Modern Aspects of Electrochemistry

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Abusive testing of large Li/SOCl2 cells

Cited by 9 publications

References 4 publications

The Lithium/Sulfuryl Chloride Electrochemical Cell

The Lithium/Sulfuryl Chloride Electrochemical Cell

Discharge Reaction Mechanisms in Li / SOCl2 Cells

Lithium Batteries with Liquid Depolarizers

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