The Electrochemical Behavior of Aluminum

Petrocelli, J. V.

doi:10.1149/1.2778129

Cited by 7 publications

(28 citation statements)

References 1 publication

(6 reference statements)

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“…In accord with the mechanism of Eq. [2] and with the dual barrier model discussed in the previous section, ~ = a~ = ~, = 1/4 and X~ X, = X, = 1. The current density of the anodic process was assumed to be of the form of Eq.…”

Section: Rtmentioning

confidence: 97%

“…[2] are assumed to be given by: alkiF ----V k~ = kl e ~T [ 7 ] ae~,2F + V ks=k~e RT [8] ----V k~=k~e RT [9] k~( +e-)…”

Section: K~(--e-)mentioning

confidence: 99%

“…[2], and X~, ~:, and X~ are the numbers of charges transferred across the interphase during the respective charge transfer steps (X~ = X~ = M = 1 is assumed in the mechanism of Eq. [2]). Substitution of Eqs.…”

Section: Cu ~ (Oxide)mentioning

confidence: 99%

“…[2], the values of P, calculated from Eq. [10] for the higher and lower potential regions of the (electrode potential)-(logarithm of current density) plot (cf.…”

Section: Rtmentioning

confidence: 99%

“…The effect of additions of oxidizable and reducible substances to solution on electrode potentials and corrosion rates of metals has been studied by several workers in recent years (2)(3)(4)(5)(6)(7)(8)(9). Numerous exploratory experiments, performed in this laboratory, have been concerned with the effect of additions of reducible ions (and some uncharged species) on the electrode potential of passive stainless steel in dilute sulfuric acid solution (3,4,9).…”

mentioning

confidence: 99%

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Kinetic Studies on Corrosion Systems

Posey¹,

Carrledge²,

Yaffe

1959

J. Electrochem. Soc.

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The reduction of cupric ion on the surface of passive stainless steel electrodes in aerated, dilute sulfuric acid medium has been investigated using potentiostatic, galvanostatic, and tracer techniques. The independent simultaneity of the electrode reactions has been demonstrated. A mechanism is advanced for the reduction of cupric ion on the oxide surface. The data are interpreted on the basis of electrochemical kinetics. * Medium: 150-400 ml of 0.105/ H2SO4 at 85~ stirred at ca. 600 rpm; pOs = 0.2 atm. Electrodes: flag-shaped type 347 stainless steel sheet electrodes (abraded surface) of 2-4 cm s geometrical area, stems lacquered with baked G. E. Glyptal. Initial electrode potentlals, before additlons, occupied region + (100-200) mv vs. S.C.E. at 25~ and were sensibly constant (+__3 mv/hr). 2.303 RT/F at 85~ = 0.071 v. 582 ) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 128.210.126.199 Downloaded on 2015-05-23 to IP Vol. 106, No. 7 ) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 128.210.126.199 Downloaded on 2015-05-23 to IP ) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 128.210.126.199 Downloaded on 2015-05-23 to IP

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Section: Rtmentioning

confidence: 97%

“…[2] are assumed to be given by: alkiF ----V k~ = kl e ~T [ 7 ] ae~,2F + V ks=k~e RT [8] ----V k~=k~e RT [9] k~( +e-)…”

Section: K~(--e-)mentioning

confidence: 99%

Section: Cu ~ (Oxide)mentioning

confidence: 99%

“…[2], the values of P, calculated from Eq. [10] for the higher and lower potential regions of the (electrode potential)-(logarithm of current density) plot (cf.…”

Section: Rtmentioning

confidence: 99%

mentioning

confidence: 99%

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Kinetic Studies on Corrosion Systems

Posey¹,

Carrledge²,

Yaffe

1959

J. Electrochem. Soc.

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Corrosion of Metals

King

1964

Recent Progress in Surface Science

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Al–Air Batteries: Fundamental Thermodynamic Limitations from First-Principles Theory

Chen

Nørskov

Luntz

2014

J. Phys. Chem. Lett.

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The Al-air battery possesses high theoretical specific energy (4140 W h/kg) and is therefore an attractive candidate for vehicle propulsion. However, the experimentally observed open-circuit potential is much lower than what bulk thermodynamics predicts, and this potential loss is typically attributed to corrosion. Similarly, large Tafel slopes associated with the battery are assumed to be due to film formation. We present a detailed thermodynamic study of the Al-air battery using density functional theory. The results suggest that the maximum open-circuit potential of the Al anode is only -1.87 V versus the standard hydrogen electrode at pH 14.6 instead of the traditionally assumed -2.34 V and that large Tafel slopes are inherent in the electrochemistry. These deviations from the bulk thermodynamics are intrinsic to the electrochemical surface processes that define Al anodic dissolution. This has contributions from both asymmetry in multielectron transfers and, more importantly, a large chemical stabilization inherent to the formation of bulk Al(OH)3 from surface intermediates. These are fundamental limitations that cannot be improved even if corrosion and film effects are completely suppressed.

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The Electrochemical Behavior of Aluminum

Cited by 7 publications

References 1 publication

Kinetic Studies on Corrosion Systems

Kinetic Studies on Corrosion Systems

Corrosion of Metals

Al–Air Batteries: Fundamental Thermodynamic Limitations from First-Principles Theory

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