Talk:Direct borohydride fuel cell
From Wikipedia, the free encyclopedia
 |
This environment-related article is part of the Environment WikiProject to improve Wikipedia's coverage of the environment. The aim is to write neutral and well-referenced articles on environment-related topics, as well as to ensure that environment articles are properly categorized. See WikiProject Environment and Wikipedia:Contributing FAQ. |
| Start | This article has been rated as Start-Class on the assessment scale. |
A form of hydrogen that is liquid at room temperature sounds like the fuel electric vehicles are looking for.
A way of boiling the water and using the steam to produce extra thrust may be useful. The waste products could be extracted from the vehicle for recycling during refuelling. Andrew Swallow Andrew Swallow 10:33, 14 September 2006 (UTC)
[edit] Standard Electrode Potential for Anode Reaction
Surely the potential for the anode reaction should be -1.24, rather than 1.24? If it were +1.24, to make the Ecell of +1.64V, the oxygen → hydroxide half-equation would be -0.4V. And in that case, the reaction would be proceed the wrong way; i.e, it would show the reduction of NaBO2, rather than the oxidation of NaBH4.
Also, if the NaBH4 half-equation has a standard electrode potential of -1.24V, then that should actually occur at the cathode, not the anode (most negative potential means oxidation, means e- produced, means -ve electrode). Nonagonal Spider (talk) 21:51, 9 May 2008 (UTC)
