Experimenteller Nachweis von Überführungswärmen in elektrolytischen Peltier‐Wärmen. (40. Mitteilung über thermochemische Untersuchungen.)

Lange, E.; Hesse, Th.

doi:10.1002/bbpc.19330390606

Cited by 3 publications

(3 citation statements)

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“…From the calculated values in Table II, the Peltier heat of the silver chloride electrode can be computed as TS%= TnF(dV/dT)t,,= 4.27 and 2.98 kcal, in 0.01N and 0.1N potassium chloride, respectively. Lange and Hesse's calorimetrically observed values are 4.52 and 3.32 kcal, respectively (22).…”

Section: Coefficients Of Electrode Potentialsmentioning

confidence: 94%

“…The experimental uncertainty in these and other observations still amounts to a few hundredths of a millivolt per degree. It seems best to assign a precision measure of not less than -----0.02 mv/deg and we shall therefore adopt, for the SHE at 25~ (dV~ +) : +0.871 -----0.02 mv/deg [22] Standard ionic entropy of electrochemical transport oI the hydrogen ion.--For the standard hydrogen electrode, the entropy of electrochemical transport S*~ is given by S *~ : S~ --2S*~ +) [23] for 2 faradays, and is equal to +0.871 mv/deg X 2F +1.742 mvF/deg ----40.17 cal/deg. Since the molal entropy of hydrogen gas is 31.211 cal/deg (6), the standard ionic entropy S*~ of H + is computed as --4.48 cal/deg --+0.5 cal/deg.…”

Section: 02m Solution ~Ic1mentioning

confidence: 99%

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The Temperature Coefficients of Electrode Potentials

deBethune

Licht

Swendeman

1959

J. Electrochem. Soc.

283

154

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The temperature coefficient of the potential of an electrode can be defined experimentally by reference to (a) the potential of the SHE at the same temperature, (b) the potential of the same electrode at some fixed temperature. These two definitions give rise to the "isothermal" and "thermal" temperature coefficients of electrode potentials. The isothermal coefficient is AS/nF where ~S is the reaction entropy of the "SHE//Electrode" cell. The thermal coefficient is S*/nF where S* is the entropy transported from the hot to the cold heat reservoir by the passage of n faradays of positive electricity through the cell from the cold to the hot electrode (before the onset of thermal diffusion). The entropy S* is divided into an entropy S*E of electrochemical transport which determines the electrode temperature effect, and an entropy S*. of migration transport which determines the thermal liquid junction potential.By assuming that S*~ is negligible in a saturated potassium chloride bridge, we have deduced that the thermal temperature coefficient of the SHE is +0.871 mv/~ [hot electrode (+) terminal] at 25~ The standard ionic entropy S* ~ of electrochemical transport of hydrogen ion is --4.48 cal/deg. Thermal temperature coefficients are computed for calomel, silver chloride, and copper sulfate electrodes and are compared with experiment. Thermal and isothermal temperature coefficients are computed and tabulated for nearly 300 standard electrode potentials.) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 132.174.255.116 Downloaded on 2015-03-10 to IP Vol. 106, No. 7 COEFFICIENTS OF ELECTRODE POTENTIALS ) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 132.174.255.116 Downloaded on 2015-03-10 to IP ) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 132.174.255.116 Downloaded on 2015-03-10 to IP

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Section: Coefficients Of Electrode Potentialsmentioning

confidence: 94%

Section: 02m Solution ~Ic1mentioning

confidence: 99%

The Temperature Coefficients of Electrode Potentials

deBethune

Licht

Swendeman

1959

J. Electrochem. Soc.

283

154

View full text Add to dashboard Cite

show abstract

“…The ionic Seebeck effect was discovered in the late 19th century 3 and the ionic Peltier effect was first accurately measured nearly a century ago. 4 The ionic Seebeck effect has been widely studied as a means of gaining insight into the fundamental thermodynamics and kinetics of electrochemical materials 5–7 and for potential applications in sensing and harvesting thermal energy. 8–14 The structure of the Li + solvation shell governs Li-ion transport and the thermodynamics and kinetics of electrochemical reactions at the electrodes.…”

Section: Introductionmentioning

confidence: 99%