Talk:Direct borohydride fuel cell

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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)[reply]

Standard Electrode Potential for Anode Reaction[edit]

Surely the potential for the anode reaction should be -1.24, rather than 1.24? If it were +1.24, to make the E_cell 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)[reply]

You are (probably) right. I'll change it. Squeezedlime (talk) 09:59, 15 August 2010 (UTC)[reply]

Accuracy dispute[edit]

NaBO₂ is sodium metaborate. Borax (sodium tetraborate) is Na₂B₄O₇.

As far as hazards go, I think sodium metaborate can be considered a mix of lye and borax. Just saying it's like borax and borax isn't very dangerous was misleading. —Preceding unsigned comment added by 75.5.10.208 (talk) 22:53, 2 April 2010 (UTC)[reply]