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Author Topic: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !  (Read 5434 times)

Offline hartiberlin

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Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« on: June 03, 2015, 04:41:02 PM »
Hi , have a look at this great new Alufoil-MnO2 battery cell with 2.67 Volts per cell ! :

https://www.youtube.com/watch?v=PLgBEUlFSiY

Hmm, I just tried to replicate this with just NaCO3 in Water instead of the NaOH at the aluminium and Epson-Salt mixed
with water and 25 % vinegar instead of the Sulfuric acid at the MnO2 side, but I only got around
1.22 Volts at maximum....

Hmm. seems I really must use these stronger chemicals to replicate it.

Probably really depends on the PH-level of these stronger alkaline base and sulfuric acid ?
I wonder how concentrated was his sulfuric acid ?

Hmm... I don´t like to play with sulfuric acid though...too dangerous..
Regards, Stefan.

Free Energy | searching for free energy and discussing free energy


Offline MarkE

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Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #1 on: June 03, 2015, 06:52:33 PM »
Hi , have a look at this great new Alufoil-MnO2 battery cell with 2.67 Volts per cell ! :

https://www.youtube.com/watch?v=PLgBEUlFSiY

Hmm, I just tried to replicate this with just NaCO3 in Water instead of the NaOH at the aluminium and Epson-Salt mixed
with water and 25 % vinegar instead of the Sulfuric acid at the MnO2 side, but I only got around
1.22 Volts at maximum....

Hmm. seems I really must use these stronger chemicals to replicate it.

Probably really depends on the PH-level of these stronger alkaline base and sulfuric acid ?
I wonder how concentrated was his sulfuric acid ?

Hmm... I don´t like to play with sulfuric acid though...too dangerous..
Regards, Stefan.
Teh sodium hydroxide to sulfuric acid  interface could be problematic due to salt precipitation.


Offline SeaMonkey

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Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #2 on: June 05, 2015, 08:06:17 AM »
That is quite interesting Stefan.

It may be possible to use Sodium Bisulfate in place of the
Sulfuric Acid.  It is available in most hardware stores as a
swimming pool additive.

Some years ago I made an aluminum-carbon cell using
a 50% solution of Chlorine Bleach mixed with water as
the electrolyte.  It produced over 2 volts and was able
to light an LED very brightly.

It is nice to know of these various ways to use aluminum
foil to make an electrical cell with readily available household
chemicals.

Offline profitis

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Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #3 on: June 12, 2015, 04:27:18 PM »
MarkE'Teh sodium hydroxide to sulfuric acid  interface
could be problematic due to salt precipitation.'

Bridge wif NaCL aq.


Offline profitis

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Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #4 on: June 12, 2015, 04:28:55 PM »
Seamonkey'It may be possible to use Sodium Bisulfate in place of
the
Sulfuric Acid'

Bingo

Free Energy | searching for free energy and discussing free energy

Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #4 on: June 12, 2015, 04:28:55 PM »
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Offline cayrex

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Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #5 on: June 16, 2015, 02:20:21 PM »
https://www.youtube.com/watch?v=8YG0nh_aYBA

My 15 min aluminium battery project from oluchem! Spec: 2.65V and 100 mA! This construction of this cell is like Daniell cell. Two metals in two different types of electrolyte (Cu in CuSO4 and Zn in ZnSO4 connected with a salt bridge).

Offline hartiberlin

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Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #6 on: June 17, 2015, 05:40:40 PM »
Very well done Cayrex !
The music is a bit too loud. But Did you say at 2:40 that you have just table salt NaCl under the aluminium ?

So what is the best configuration yet ?

Can you try to light a few yellow and green LEDs with it ?

At around 250 MilliWatts output of such a cell these LEDs should be really bright !

How strong was your H2SO4 acid ? Did you just use car battery acid or stronger ?

Did you try to recharge the cell ? Does this work ? For recharging it is probably the best to have
AlCl3 electrolyte at the aluminiumfoil to put the Aluminium ions back onto the foil...

Did you have a graphite plate ontop of the MnO2 ? Or did you just use the MnO2 powder only ?
Many thanks.

Regards, Stefan.

Free Energy | searching for free energy and discussing free energy

Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #6 on: June 17, 2015, 05:40:40 PM »
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Offline profitis

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Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #7 on: June 17, 2015, 07:04:29 PM »
Boss'Did you try to recharge the cell ? Does this work ? For
recharging it is probably the best to have
AlCl3 electrolyte at the aluminiumfoil to put the
Aluminium ions back onto the foil...'

Unfortunately aluminum anodes in aquaeous chemistry is total irreversible.no aluminum plates out frm Al sols.you want to try zinc anode in NaOH for moderate reversability.you want to try KNO3/H2SO4 or K2Cr2O7/H2SO4 aq. with carbon rod for potent cathode.

Offline cayrex

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Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #8 on: June 17, 2015, 10:42:41 PM »
Very well done Cayrex !
The music is a bit too loud. But Did you say at 2:40 that you have just table salt NaCl under the aluminium ?

So what is the best configuration yet ?

Can you try to light a few yellow and green LEDs with it ?

At around 250 MilliWatts output of such a cell these LEDs should be really bright !

How strong was your H2SO4 acid ? Did you just use car battery acid or stronger ?

Did you try to recharge the cell ? Does this work ? For recharging it is probably the best to have
AlCl3 electrolyte at the aluminiumfoil to put the Aluminium ions back onto the foil...

Did you have a graphite plate ontop of the MnO2 ? Or did you just use the MnO2 powder only ?
Many thanks.

Regards, Stefan.

Uf,... so many questions  ;D :P

Orginal setup: Chatode: MnO2 and graphite in H2SO4, Anode: Al in NaOH and  in the middle Na2SO4 because of the reaction NaOH + H2SO4 = Na2SO4 + H2O

the salt which I use is the side product from my reaction  CoCl2 + NaOH -> Co(OH)2 + NaCl. Co(OH)2 was at the bottom and NaCl on the top,.... I use the liquid on the top (possible may contain some cobalt atoms). try with concentrated NaCl. best configuration,.... hmm,... I think, two difrent salts or AlCl3 on - and H2SO4 on +. I try a green LED and 3V electric motor,.... work realy good. I use 15 - 20% of H2SO4.

Did you try to recharge the cell ? no,... the Al is in 60 min realy bad damaged in alone in siting in NaOH. With this setup is no option to recharge the cell. I think will possible work,... with Al-GIC/AlCl4-ion l. (aluminium ion electrode in aluminium salt/ionic, DES,...) but this is more complex concept ;)

Also in this project I use a zinc and magnesium. MnO2 - Mg: 2.42V and MnO2 - Zn: 2.40V

Offline profitis

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Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #9 on: June 18, 2015, 12:49:56 PM »
Crayex' MnO2 and graphite in H2SO4,'

Alternative is to plate MnO2 direc onto carbon rod from MnSO4/H2SO4 aq. Then use this partially immerse in NaOH sol as exellent oxygen/air catalyst electrode.couple with Zn anode in NaOH and no need for current-limiting saltbridge.makes quite reversible cell aprox 2v.

Free Energy | searching for free energy and discussing free energy

Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #9 on: June 18, 2015, 12:49:56 PM »
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Offline SeaMonkey

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Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #10 on: June 26, 2015, 07:10:27 AM »
We must not forget that the Manganese Dioxide (MnO2)
is a Depolarizer that is chemically changed as the cell
produces electrical current.  Without this depolarizer
Hydrogen bubbles would collect on the surface of the
positive electrode thereby increasing the internal
resistance of the cell and diminishing its ability to
produce electrical output.

Offline profitis

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Re: Alufoil-MnO2 Battery cell with 2.67 Volts ! WOW !
« Reply #11 on: June 27, 2015, 09:41:13 AM »
In acid: Mno2 + 4H+ + 4e-> Mn2+ + 2h2o E= 1.23v

In alkali: Mno2 + 2h2o + 2e- > Mn(oh)2 + 2oh- E= 0.1v

in alkali, oxygen/air can reverse the above reaction because O2 + 2h20 + 4e-  > 4OH- E= 0.414v   higher than 0.1v


 

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