HUSCAP logo Hokkaido Univ. logo

Hokkaido University Collection of Scholarly and Academic Papers >
Graduate School of Engineering / Faculty of Engineering >
Peer-reviewed Journal Articles, etc >

Chemical equilibrium analysis for hydrolysis of magnesium hydride to generate hydrogen

Files in This Item:
IJHE37-17_12114-12119.pdf502.39 kBPDFView/Open
Please use this identifier to cite or link to this item:

Title: Chemical equilibrium analysis for hydrolysis of magnesium hydride to generate hydrogen
Authors: Hiraki, Takehito Browse this author
Hiroi, Shun Browse this author
Akashi, Takuya Browse this author
Okinaka, Noriyuki Browse this author
Akiyama, Tomohiro Browse this author →KAKEN DB
Keywords: Hydrolysis
Equilibrium analysis
Magnesium hydride
Buffer capacity
Issue Date: Sep-2012
Publisher: Elsevier
Journal Title: International Journal of Hydrogen Energy
Volume: 37
Issue: 17
Start Page: 12114
End Page: 12119
Publisher DOI: 10.1016/j.ijhydene.2012.06.012
Abstract: Magnesium hydride is a promising hydrogen source because of its high mass density of hydrogen, 15.2%, when it is hydrolyzed; MgH2 + 2H2O = Mg(OH)2 + 2H2 + 277 kJ. However, a magnesium hydroxide, Mg(OH)2, layer forms rapidly on the surface of the unreacted MgH2 as the pH increases, hindering further reaction. The purpose of this study is to find acids that could effectively accelerate the reaction by using a chemical equilibrium analysis where the relationships of pH to concentration of ionized Mg were calculated. For the best performing acid, the calculated and measured relationships were compared, and the effects of acid concentration on hydrogen release were measured. The analysis revealed that citric acid and ethylenediamine-tetraacetic acid were good buffering agents. The calculated and measured relationships between pH and concentration of ionized Mg were in good accord. Hydrogen release improved considerably in a relatively dilute citric acid solution instead of pure distilled water. The maximum amount of hydrogen generated was 1.7 x 10^[3] cm3・g^[-1] at STP after 30 min. We estimated the exact concentration of citric acid solution for complete MgH2 hydrolysis by a chemical equilibrium analysis method.
Type: article (author version)
Appears in Collections:工学院・工学研究院 (Graduate School of Engineering / Faculty of Engineering) > 雑誌発表論文等 (Peer-reviewed Journal Articles, etc)

Submitter: 秋山 友宏

Export metadata:

OAI-PMH ( junii2 , jpcoar_1.0 )

MathJax is now OFF:


 - Hokkaido University