The Characterization of Internal Power Losses in Pacemaker Batteries by Calorimetry

Hansen, Lee D.; Hart, R. M.

doi:10.1149/1.2131565

Cited by 23 publications

(13 citation statements)

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“…It is assumed that there are several simultaneous electrode reactions of the form (6) occurring within the battery. The reactions are written so that species i is always in a phase type m, baving a certain secondary reference state.…”

mentioning

confidence: 99%

A General Energy Balance for Battery Systems

Bernardi

Pawlikowski

Newman

1985

J. Electrochem. Soc.

1,598

604

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mentioning

confidence: 99%

A General Energy Balance for Battery Systems

Bernardi

Pawlikowski

Newman

1985

J. Electrochem. Soc.

1,598

604

View full text Add to dashboard Cite

“…Therefore, the exponential model as given in Eq. [1] is assumed to describe the kinetics of the open-circuit reaction qoc = -A Uktt x [ 1 ] a Uncertainties are given as the standard deviation of the parameter as obtained from the least squares fit of a linear equation to all of the data.…”

Section: Resultsmentioning

confidence: 99%

“…The calorimeter used during most of the study was a Tronac Model 351 RA (1). The constant temperature bath in this calorimeter has an upper limit of 45~ Therefore, when measurements were made at temperatures above 45~ with this instrument, the calorimeter measuring unit was moved to a Hart Scientific Model 5024 water bath.…”

Section: Equipmentmentioning

confidence: 99%

Kinetics and Thermodynamics of Chemical Reactions in Li / SOCl2 Cells

Hansen

Frank

1987

J. Electrochem. Soc.

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The kinetics of the heat producing processes in undischarged and partially discharged Li/SOC12 cells under open-and closed-circuit conditions have been measured by heat conduction microcalorimetry. The cells studied, Honeywell Type G2666 reserve cells, were activated as needed, and the rates of open-and closed-circuit heat output were determined as a function of time since activation, temperature, and state of discharge. The results of the open-circuit measurements on whole cells are described by an equation of the form q = hUkt x where q is the rate of heat output, AU is the heat produced per unit of reaction, k and x are empirical constants, and t is the time since activation. Both x and k are found to be functions of temperature. Heat producing processes occur at both the anode and cathode under open-circuit, undischarged conditions, but the processes at the carbon cathode produce only a few percent of the total heat. The state of discharge has only a small effect on the open-circuit rate of heat production. Withdrawing current from Li/SOCl~ cells greatly increases the rate of heat output from noncurrent producing reactions. At short times after activation (i.e., <200h) and at high temperatures, the heat produced by nonfaradaic processes can be several times as large as the heat produced by external current being drawn from the cell. At short times after activation, the excess heat is probably due to corrosion of Li, and, at long times after activation, the excess heat is probably due to the reaction of a long-lived intermediate in the cell electrolyte. A thermodynamic analysis of the cell gives values ofhH~ of -374.1 -+ 0.5 (25~ and -376 +-1 (65~ k J/equivalent and values ofhS~ of -75 + 1 (25~ and -71 + 3 (65~ J/K-equivalent, where hH~ and AS~ are the enthalpy and entropy changes for the cell reaction occurring at the electrodes.Shelf-life testing of primary batteries is often done at elevated temperatures in order to shorten the time required for the tests. The results at the elevated temperature are then extrapolated to room temperature. The results of such a procedure are valid provided that no change in the mechanism of the parasitic processes occurs between room temperature and the temperature at which the tests are done. The work described in this report was designed to determine the kinetic constants necessary for the extrapolation of kinetic data on Li/ SOC12 cells over the temperature range from 25 ~ to 75~A second objective of the work described in this report was to characterize as far as possible the chemical reactions that occur in Li/SOClz cells since these reactions may be important in understanding the potential hazards of these cells.The specific objectives of the work done in this study are (a) to determine the kinetics of the corrosion processes in undischarged Li/SOC12 cells, (b) to separate the kinetics of the corrosion processes occurring at the anode and cathode, (c) to determine the effects on corrosion reactions of switching current on and off, and (d) to determine the effect...

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“…The rate of loss of that energy, and hence the lifetime of the battery, may be determined by simply inserting the battery into an isothermal calorimeter. 71 This principle is the basis for calorimetric quality control tests now routinely done on batteries to be used in critical applications such as heart pacemakers and satellites. Corrosion of battery materials under both open-and closed-circuit conditions can also be studied by isothermal calorimetry.…”

Section: Illustrative Examples Of Applicationsmentioning

confidence: 99%

Calorimetric Measurement of the Kinetics of Slow Reactions

Hansen

2000

Ind. Eng. Chem. Res.

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A brief review of the application of calorimetry to measurement of the kinetics of slow processes is presented. Processes degrading or otherwise changing the properties of materials often occur too slowly to be readily measured by conventional chemical analyses but can be measured in a relatively short period of time by heat conduction calorimetry. Instrument selection and derivation of rate laws from calorimetric data are discussed, and illustrative examples are presented.

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The Characterization of Internal Power Losses in Pacemaker Batteries by Calorimetry

Cited by 23 publications

References 1 publication

A General Energy Balance for Battery Systems

A General Energy Balance for Battery Systems

Kinetics and Thermodynamics of Chemical Reactions in Li / SOCl2 Cells

Calorimetric Measurement of the Kinetics of Slow Reactions

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