Aluminum and aluminum alloys as sources of hydrogen for fuel cell applications

Soler, Lluís; Macanás, Jorge; Muñoz, Marı́a; Casado, Juan

doi:10.1016/j.jpowsour.2007.01.080

Cited by 271 publications

(109 citation statements)

References 20 publications

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“…According to Deng and Ferreira (2007), the formation of several intermediates, such as pseudoboehmite (AlOOH), can be predicted from a mathematical model of the critical pressure of hydrogen bubbles inside the passivation layer of oxide. The addition of NaAl(OH) 4 , the replacement of NaOH by NaAlO 2 and the addition of other compounds such as salts has been described in the literature (Soler et al, 2007(Soler et al, , 2009, and all give similar results for the yields and reaction rates.…”

Section: Introductionmentioning

confidence: 68%

“…When metallic elements from groups IA and IIA of the periodic table come in contact with water (e.g., Na, K, Li) the corresponding metal hydroxide and hydrogen are formed. Such a reaction only proceeds with aluminum in the presence of a strong alkaline compound, such as NaOH or KOH (Soler et al, 2009;Soler et al, 2007) because this metal has a very thin passive layer of Al 2 O 3 on its surface that prevents the direct attack of water molecules (Grosjean et al, 2005;Wang et al, 2009). The reaction between aluminum and water can occur in the absence of any alkali if special alloy elements (e.g., indium and gallium) are added to aluminum in small quantities (Parmuzina et al, 2008;Kravchenko et al, 2005;Dow et al, 1997).…”

Section: Introductionmentioning

confidence: 99%

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Production of hydrogen in the reaction between aluminum and water in the presence of NaOH and KOH

Porciúncula¹,

Marcílio²,

Tessaro³

et al. 2012

Braz. J. Chem. Eng.

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-The objective of this work is to investigate the production of hydrogen as an energy source by means of the reaction of aluminum with water. This reaction only occurs in the presence of NaOH and KOH, which behave as catalysts. The main advantages of using aluminum for indirect energy storage are: recyclability, nontoxicity and easiness to shape. Alkali concentrations varying from 1 to 3 mol . L -1 were applied to different metallic samples, either foil (0.02 mm thick) or plates (0.5 and 1 mm thick), and reaction temperatures between 295 and 345 K were tested. The results show that the reaction is strongly influenced by temperature, alkali concentration and metal shape. NaOH commonly promotes faster reactions and higher real yields than KOH.

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Section: Introductionmentioning

confidence: 68%

Section: Introductionmentioning

confidence: 99%

Production of hydrogen in the reaction between aluminum and water in the presence of NaOH and KOH

Porciúncula¹,

Marcílio²,

Tessaro³

et al. 2012

Braz. J. Chem. Eng.

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“…The aluminum alloys that are presently lost in bottom ash treatment plants may form the largest single loss in the whole aluminum cycle [1][2][3]. According to some estimates, approximately 1.52 million tons of aluminum alloy with a high pure aluminum content is used annually for packaging cans in Europe [4].…”

Section: Introductionmentioning

confidence: 99%

Recovery of Aluminum Residue from Incineration of Cans in Municipal Solid Waste

Hu¹,

Bakker²

2015

JRST

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ABSTRACT:The interest to investigate to which degree aluminum residue from cans may be recovered from MSWI bottom ash. To this end an assessment was made of the cans residue size distribution in bottom ash and its potential for recovery. This study indicates that nonferrous concentrates from Amsterdam bottom ash contain interesting amounts of aluminum cans residue (0.055% of the ash). About 61.7% of the input of aluminum cans are ended after combustion in the 6-20 mm ash fraction. Also it is shown that a combination of dry and wet separation can improve aluminum residue recovery with respect to the single dry process.

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“…The presence of the catalyst (strong alkali, NaOH and KOH) is necessary because the reaction of the metal with water does not occur due to presence of a very thin passivation layer, Al 2 O 3 , which hinders the reaction ( [6] e [3]). The use of alkalis, like NaOH and KOH, promotes the complete removal of this layer, so that the reaction with water may proceed ( [4], [5]). The reaction that occurs is as follow:…”

Section: Introductionmentioning

confidence: 99%

“…In [8], the formation of an intermediate (pseudoboehmite, AlOOH) was considered in a mathematical approach that accounts for the pressure of the hydrogen bubbles formed under the metal surface, thickness of the hydrated oxide film, and other effects. Also, NaAl(OH) 4 was considered an intermediate compound, and the replacement of NaOH by NaAlO 2 as catalyst was successfully verified ( [4], [5]). …”

Section: Introductionmentioning

confidence: 99%

Hydrogen production by aluminium corrosion: experimental investigation and mathematical modelling

Porciúncula¹,

Marcílio²,

Tessaro³

et al. 2011

REPQJ

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Abstract. The search for new energy sources has been a great focus lately because of concerns about climate change caused mainly by fossil fuels gas emissions. The hydrogen is a promising energy source due its clean and high energy combustion. However, the major drawbacks to use hydrogen are the difficulty of formation, transportation and storage. The objective of this work is the study of hydrogen formation by aluminium reaction with water by using strong alkalis as catalysts (NaOH and KOH), and the development of a mathematical model that accounts the evolution of hydrogen at each time. Different alkali concentrations were used (1, 1.5, 2, 2.5 and 3 mol . L -1 ). The reactions were carried out with aluminum in different samples: foils, plates with 0.5 mm and 1 mm width each. The range of temperatures studied was: 295, 305, 315 and 325 K for foils and 0.5 mm plates; 315, 325, 335 and 345 K for 1 mm plates. The results show ed a strong dependence of the reaction rate on the temperature, alkali concentration and shape of the samples. The model predictions of hydrogen formation agreed with the experimental data of volume versus time, as well as the peaks observed in the reaction rates.

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Aluminum and aluminum alloys as sources of hydrogen for fuel cell applications

Cited by 271 publications

References 20 publications

Production of hydrogen in the reaction between aluminum and water in the presence of NaOH and KOH

Production of hydrogen in the reaction between aluminum and water in the presence of NaOH and KOH

Recovery of Aluminum Residue from Incineration of Cans in Municipal Solid Waste

Hydrogen production by aluminium corrosion: experimental investigation and mathematical modelling

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