Viscosité des gaz et données critiques

Sabatier, Germain

doi:10.1051/jcp/1951480113

Cited by 7 publications

(6 citation statements)

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“…At elevated temperatures decomposition of the nitrate to oxide or nitrite occurs; no nitrite is ever formed directly. This is the course of reaction with, for example, sodium (28,199,344), potassium, zinc (15,21,23), silver (115, 293), and lead (344). It is the reaction which occurs when nitrogen dioxide attacks the surface in a mercury manometer to form mercurous and mercuric nitrates (15,21,23,115,293).…”

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confidence: 99%

“…Reaction at high temperatures At high temperatures metals react to yield a mixture of products, many of which may be derived from decomposition of nitrate formed initially in the manner described, but some of which are more likely the result of oxidation by nitrogen dioxide. Thus, potassium burns with a red flame, forming nitrite as well as nitrate (115, 293); magnesium is oxidized at dull-red heat (344); and manganese, iron, cobalt, and nickel are oxidized (344). The increased rate of reaction of zinc with dinitrogen tetroxide above 14°C.…”

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confidence: 99%

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The Reactivity And Structure Of Nitrogen Dioxide

Gray¹,

Yoffe²

1955

Chem. Rev.

131

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confidence: 99%

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confidence: 99%

The Reactivity And Structure Of Nitrogen Dioxide

Gray¹,

Yoffe²

1955

Chem. Rev.

131

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“…For example, the water supplies the hydrogen to generate H 2 in neutral and alkaline environment, which thus requires the electrocatalyst with good ability of water adsorption and dissociation to reactive hydrogen intermediates (H*) at rate‐limiting Volmer step (H 2 O + e → H* + OH − ) of the HER . In acidic media, efficient adsorption of the protons (H + ) on the electrocatalyst should be taken into the consideration since they supply the hydrogen to trigger the HER . In all cases, a nearly zero Gibbs free energy of H* adsorption (∆ G H* ) is necessary to moderate the H* binding strength on catalyst surface, which accelerates the HER without suppressing H 2 release according to the Sabatier principle .…”

Section: Introductionmentioning

confidence: 99%

“…In acidic media, efficient adsorption of the protons (H + ) on the electrocatalyst should be taken into the consideration since they supply the hydrogen to trigger the HER . In all cases, a nearly zero Gibbs free energy of H* adsorption (∆ G H* ) is necessary to moderate the H* binding strength on catalyst surface, which accelerates the HER without suppressing H 2 release according to the Sabatier principle . Fast mass/charge transport at liquid–solid–gas interface and high robustness against distinct pH conditions are also critical to full exploitation of intrinsic properties of the catalyst toward HER.…”

Section: Introductionmentioning

confidence: 99%

Engineering Multifunctional Collaborative Catalytic Interface Enabling Efficient Hydrogen Evolution in All pH Range and Seawater

Zhao

Wang

et al. 2019

Advanced Energy Materials

244

135

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Developing electrocatalysts with high compatibility to the reaction systems with complicated chemical properties represents an important frontier of catalyst design. Herein, a strategy by engineering a multifunctional collaborative catalytic interface to propel the hydrogen evolution reaction (HER) in the full pH range and seawater is reported. Collaborative catalytic interfaces among MXene, bimetallic carbide, and hybridized carbon are demonstrated to afford overall enhancement in electrical conductivity, exposure of reactive sites, water dissociation kinetics, H+/water adsorption, and intermediate H binding capability, which satisfy highly variable chemical environment for HER under different pH conditions. Therefore, the HER performance of resultant electrocatalysts can compete with commercial Pt/C in 0.5 m H2SO4 or 1.0 m KOH but outperform it under pH 2.2–11.2. They also show exceptional performance for HER in natural seawater with stringent requirements in catalytic activity and stability, exhibiting the best combination of Pt‐like activity, long durability (225 h, 64 times that of Pt/C), and 98% Faradaic efficiency, comparable with commercial Pt/C and the best documented electrocatalysts by far. This work may shed fresh light into the design of effective electrocatalytic interface for regulating the energy chemistry over wide operation conditions, and also inspires the exploration of hydrogen energy utilization technologies and beyond.

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“…2 hydrate as given by temperature-scanning thermograms are displayed in the pressure-temperature diagram inFigure 3, for the purpose of comparison.When the particle size is chosen to be ca [3][4][5]. Temperature range ca.…”

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confidence: 99%

Mechanisms and kinetics of the thermal decomposition of sodium sulphide pentahydrate under controlled water vapour pressure

Andersson¹,

Azoulay²

1986

J. Chem. Soc., Dalton Trans.

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The kinetics and mechanism of the thermal decomposition of sodium sulphide pentahydrate to an essentially anhydrous form was investigated, in the pressure range 3-20 Torr, using thermogravimetry and X-ray powder diffractometry under controlled temperature and water vapour pressure. A two-step dehydration reaction pathway involving an intermediate dihydrate phase was observed: Na2S=5H,0 --+ Na2S2H20 + 3H20 (9); Na2S*2H,0 --+ Na2S + 2H,O (9). The latter reaction is shown t o be relatively more inhibited than the first. The intermediate phase was studied by means of simultaneous thermogravimetry and X-ray powder diffraction methods. A structural transformation is proposed in terms of a topotactic process, which readily accounts for the readiness with which the first reaction takes place and which is also consistent with the overall structural transformation from the pentahydrate to the anhydrous product.A wide variety of hydrated sodium sulphide species has been quoted in the literature as being formed either by crystallization from solutions or by thermolysis in the solid state.' The Occurrence of Na2S*9H,0 is acertained beyond doubt, whereas for the lower hydrates a number of controversial results are found in the literature.In their solubility studies, Parravano and Forniani claimed the existence of a hexahydrate and a 5.5 hydrate in the temperature ranges 48-91.5 and 91.5-94 "C. The latter hydratewasalso found tobemetastablebetween48.9and91.5 "C.Using various different preparative procedures, Bottger,3 Sabatier,4 and Lemoine obtained a pentahydrate, Na2Se5H,0. Later on, Sanfourche described an intermediate stable above 85 "C, which was supposed to be a monohydrate. In a more n = I3.34(m/m,) -4.34(3)

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Viscosité des gaz et données critiques

Cited by 7 publications

References 0 publications

The Reactivity And Structure Of Nitrogen Dioxide

The Reactivity And Structure Of Nitrogen Dioxide

Engineering Multifunctional Collaborative Catalytic Interface Enabling Efficient Hydrogen Evolution in All pH Range and Seawater

Mechanisms and kinetics of the thermal decomposition of sodium sulphide pentahydrate under controlled water vapour pressure

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