Infrared Absorption Coefficients for Certain Pollutant Gases

Campani, P.; Fang, Chonghua; Prengle, H. W.

doi:10.1366/000370272774352119

Cited by 12 publications

(6 citation statements)

References 43 publications

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“…However, at potentials higher than 4.7 V, a pronounced CO 2 and CO evolution is detected by these in situ spectroelectrochemical studies. Using the known spectral absorption coefficients for CO 2 ͑at 2349 cm −1 ͒ and CO ͑at 2174 cm −1 ͒, 16 we estimated the absolute quantity of CO 2 and CO gases that typically evolve during a whole CV cycle in the cell described above. The results are shown in Table II.…”

Section: Resultsmentioning

confidence: 99%

In Situ FTIR Spectroscopy Study of Li/LiNi[sub 0.8]Co[sub 0.15]Al[sub 0.05]O[sub 2] Cells with Ionic Liquid-Based Electrolytes in Overcharge Condition

Sharabi¹,

Markevich²,

Borgel³

et al. 2010

Electrochem. Solid-State Lett.

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We developed a methodology of in situ Fourier transform infrared ͑FTIR͒ measurements of gaseous products formed in an electrochemical cell upon polarization. LiNi 0.8 Co 0.15 Al 0.05 O 2 ͑NCA͒ cathodes were explored at potentials of up to 5.5 V vs Li in the ionic liquid ͑IL͒-based electrolyte solution, LiTFSI/N-butyl-N-methylpyrrolidinium bis͑trifluoromethanesulfonyl͒amide. The polarization of the NCA electrodes formed CO 2 and CO due to the liberation of oxygen and the parallel dissolution of nickel ions, which oxidizes the carbon black in the composite electrode. The oxygen was mostly liberated from the NCA and also due to minor contribution from the surface groups on the carbon black additive.The possible development of internal pressure is one of the most serious safety problems of Li-ion batteries, especially for large applications such as electric vehicles. The development of overpressure due to the gas evolution in side reactions can break the hermetically sealed housing of the battery. Exposure of the reactive battery components to air can then lead to fire and explosions. 1-3 Internal pressure can develop upon storage at elevated temperature 2,4-6 and when the battery is overcharged. 1,7,8 The safety of lithium-ion batteries under overcharge conditions is determined by the thermal behavior and by the nature and quantity of gases that can be generated by them.LiNi 0.8 Co 0.15 Al 0.05 O 2 ͑NCA͒ is a promising cathode material for lithium-ion batteries because of its higher specific capacity and lower cost compared to LiCoO 2 . Gas evolution with NCA cathodes as a function of temperature, voltage, and the presence of additives in conventional electrolyte solutions based on alkyl carbonates has already been studied. 2,4,6 The main gaseous compound that was formed at positive electrodes in conventional electrolyte systems was CO 2 , for which several mechanisms of formation in these systems can be drawn. A main source of CO 2 is the oxidative decomposition of the carbonate solvents or surface films containing carbonate groups on the positive electrode. 4,5 Another possibility for gas evolution in these systems is the degradation of the overcharged cathode material. [6][7][8] To discriminate between these processes during the storage of charged Li-ion cells at elevated temperatures, Onuki et al. employed 13 C-labeled organic carbonate solvents and showed that 37% of CO 2 evolution in extreme situations cannot be related to solvent decomposition, but rather to the carbon present in the composite electrode as a conductive additive, or to the binder. In recent years, there have been efforts to introduce ionic liquids ͑ILs͒ as main solvents or critical solution components into Li-ion batteries because of their apparent high anodic stability and promising safety features: nonvolatility, nonflammability, and expected high thermal stability. 9,10 ILs based on cations that are derivatives of pyrrolidinium are especially important because of their relatively high cathodic stability ͑they may be compatible with Li metal...

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Section: Resultsmentioning

confidence: 99%

In Situ FTIR Spectroscopy Study of Li/LiNi[sub 0.8]Co[sub 0.15]Al[sub 0.05]O[sub 2] Cells with Ionic Liquid-Based Electrolytes in Overcharge Condition

Sharabi¹,

Markevich²,

Borgel³

et al. 2010

Electrochem. Solid-State Lett.

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“…self-broadening coefficient K absorption coefficient, em -I L pathlength, em (f Stefan-Boltzmann coefficient (-5.669 x n self-broadening exponent 10- 12 [7][8][9][10]. The purpose of the present work is to perform a similar type of study on ethylene (e 2 " ,) , which is also one of the primary decomposition products evolved from the pyrolization of condensed fuels.…”

Section: Nomenclaturementioning

confidence: 99%

“…The purpose of the present work is to perform a similar type of study on ethylene (e 2 " ,) , which is also one of the primary decomposition products evolved from the pyrolization of condensed fuels. Highresolution spectroscopic studies on the infrared radiation properties of ethylene have received considerable attention in the past [11][12][13][14][15]. These studies are useful for determining the concentrations of air pollutants in the atmosphere and for other low-absorber concentration analysis.…”

Section: Nomenclaturementioning

confidence: 99%

Infrared Radiation Properties of Ethylene

Tuntomo

Park

Tien

1989

Experimental Heat Transfer

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Quanti/alive analysis of the effect of radialive energy blockage during the combustion process of condensed fuels requires a knowledge of the infrared radialion properties of various hydrocarbon gases as a function of temperature and optical pathleng/h. The spectral absorptivities of the four infrared-active bands of ethylene (CzH.J have been measured at low resolution for temperatures between 300 and 700 K. These measurements have been used to correlate both the spectral-mean parameters and the wide-band parameters for each of the four major bands in the infrared region. The spectral-mean parameters have been determined from the stalistical narrow-band model, while the wide-band parameters have been obtained from the Edwards exponential wide-band model. The wide-band parameters have been further utilized for the development of both the total emissivity and the Planck mean absorption coefficient charts. In addition, based on the Tien-Brosmer super-band model, the super-band parameters have also been determined in the present work for convenient engineering applicalion.

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“…As part of this project, Campani et al (1972) measured fcp-values, required for Equation 14, for a number of pollu- ('-vibrational rotational band, P&R branches R-branch used, maximum at 2170 cm-1 approx. Herzberg, 1939Banwell, 1966Pierson et al, 1956 n Av =!…”

Section: Pollutant Concentration Measurementmentioning

confidence: 99%