Intro
Intro: Bleaching Powder Battery
Its a simple homemade battery costs around .92$
1
Step 1: Materials
500g of ordinary chlorax bleachTap water×1 clip cable×10 50ml small container's×10 aluminum strips×10 copper stripsmultiple voltametre
2
Step 2: Cells Construction
Take a knife , make two slits , beware make one small and make one bit large and make a small hole using shouldering iron for drain hole.
3
Step 3: Electrodes
Fit the aluminium strip to the large slit and copper to small slit.ALUMINUM - cathodeCOPPER + anode
4
Step 4: Filling Electrolyte
Take one container, fill water until it reaches top, later add a spoon of chloride bleach, stirred it well until it dissolve.
5
Step 5: Testing Cell
Have a look, each cell produces around 1.35v to 1.45v.
6
Step 6: Connecting All Cells
Now, I have connected all cells together, it produces 14.30v to around 15v max so I can easily connect to my home theater.THANK YOU...............
Step 1: Materials
500g of ordinary chlorax bleach
Tap water
×1 clip cable
×10 50ml small container's
×10 aluminum strips
×10 copper strips
multiple voltametre
Tap water
×1 clip cable
×10 50ml small container's
×10 aluminum strips
×10 copper strips
multiple voltametre
Step 2: Cells Construction
Take a knife , make two slits , beware make one small and make one bit large and make a small hole using shouldering iron for drain hole.
Step 3: Electrodes
Fit the aluminium strip to the large slit and copper to small slit.
ALUMINUM - cathode
COPPER + anode
ALUMINUM - cathode
COPPER + anode
Step 4: Filling Electrolyte
Take one container, fill water until it reaches top, later add a spoon of chloride bleach, stirred it well until it dissolve.
Step 6: Connecting All Cells
Now, I have connected all cells together, it produces 14.30v to around 15v max so I can easily connect to my home theater.
THANK YOU...............
THANK YOU...............
<p>I would seriously like to know how this type of knowledge is obtained. The contributors and commenters, (while not always the best spellers) have a grasp of chemistry, physics, engineering, etc. that I never got in school and I know my kids are not getting, despite taking AP Science classes. Without practical application, there is little retention or deep understanding of complex connections, but even simple applications that could lead to more innovation. Is this by design? Because I feel that if more kids were exposed to the exciting world of making, and doing, with mentors who encouraged trial and error, but supervised to teach safety, to prevent accidents, we would see much more engaged citizens and less crime even. Yet the schools and local governments seem resistant to allow the development of spaces that would nurture this type of learning.</p>
<p>very, very interesting... my self and my grandsons would try this ....will use led on the output or led bulbs according to voltage...maybe it will make a good night light...i bought a led clock that has a wick and uses water to power it,its over a year now and it is still working.</p>
thanks
<p>my great grandfather had a 12' x 16' poured concrete vat 4' high in the side yard of his house around 1931?- 1953 (a-c lines finally ran to area). this vat contained similar cathodes and water with an active agent from U.S.Carbide added a 90 pound bag at the time.my mother can verify this but did not know name of agent used.</p>
<p>US Carbide is an acetylene manufacturer, so that bag was more than likely calcium carbide, like the name. Coal miners use to wear CC lamps, where they'd drop a lump into some water for light down below.</p>
Wow, amazing, the next step is making it rechargeable somehow...
IT IS NOT RECHARGEABLE, <br> if you try to recharge the electrodes may carrode ,<br><br>IF YOU WANT TO MAKE A RECHARGEABLE BATTREY,<br> Just fill the cells with salt water and charge with 24v output charger.
<p>Please, tellme more.</p>
<p>Don't do this (@home)!<br>You will get H2 + 1/2*O2 which could be explosive.</p>
<p>I think you mean "corrode" :)</p>
this is ingenious man, im very impressed, well done my friend, well done
<p>How long do they last? How do you recharge them? Any 'under load' current readings?</p>
IT IS NOT A RECHARGEABLE BATTREY.......<br> If you try to attempt charging the electrodes "CARRODE".
<p>hello dear,</p><p>grate work at this what is the amps value when you make it you check ?????</p><p> (short circuit current) ?????</p>
<p>I think the word you are trying to spell is "CORRODE".</p><p>Chlorine-based electrolyte solution might be corrosive on its own. Is it not? It doesn't appear that the electrodes would last that long unless you are aiming to make a disposable battery. In that case it would do.</p>
If you notice low voltage.....<br>Don't worry, just drain the water and refill new electrolyte.
How long will this battery lasts for a volatge more than 12v..??
if the surface area is increased, you may be able to get more voltage per cell...
<p>The increased surface area would provide more amps, right?</p>
Couldn't tell you for sure, I don't know a lot about battery chemistry, should provide more energy density... Would think that it would provide a higher voltage.
<p>the voltage per cell is determined by potentials of the two metals and their respective electrolytes. I believe if the electrolyte is the same on both sides, then it's just a matter the difference of the two metal's respective potentials (vague memories of Junior high science class).</p><p> See http://en.wikipedia.org/wiki/Standard_electrode_po... <br><br>Greater area provides greater potential current as per the obvious thought experiment.</p>
<p>If anyone looked at the link from ericCycles,can you explain this chart to me?:</p><p>http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page)</p><p>I'm wanting to figure out which 2(I'm guessing you would call them "opposites")would make the best electrodes?Basically I want to experiment with voltage/current differentials for various metals I may have laying around.Thanks!</p>
<p>For an explanation, see the page <a href="http://www.electrical4u.com/voltaic-cell/" rel="nofollow">http://www.electrical4u.com/voltaic-cell/</a> </p><p>But as I recall my junior high chemistry class, the voltage of the cell is going to be the difference between the two electro potentials of the metals used. From the table, Aluminum (al) has -1.66 and Tin (Sn) has 0.15, so substract the two potentials and you have 1.81V (ignoring the sign). My chemistry is way too rusty to remember how to handle things like copper which has multiple valances. If you try the experiment, remember to use pure metals rather than alloys since that would be a much more complicated set of chemical reactions to try to figure out. I'm guess that the chunk of aluminum the original author used was probably an alloy because from the table, I would have expected a higher voltage than 1.38. </p>
<p>Thanks,I guess that's what I'm trying for.For example,if I used,say Aluminum and,oh,I dunno,Bismuth for electrodes,will it give a higher or lower voltage output than,say,Aluminum and Silver,given the same mass?I'm assuming(even though it's dangerous),that the size of the electrodes controls current potential(asside from paralleling cells)?This is all brand new to me,so any input is appreciated!</p>
<p>As Rand0mUser says. Putting cells in parallel is equivalent to getting greater surface area, and hence greater possible current draw. The voltage is determined by the nature of the chemical reaction (ie, the metals an electrolytes used). This page has an interesting explanation of why actual voltages differ: <a href="http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/electrode.html" rel="nofollow">http://hyperphysics.phy-astr.gsu.edu/hbase/chemica...</a><br> As for aluminum, silver, and bismuth, the table already references awaits you, it's simple subtraction.</p>
<p>Thanks again ericCycles,for another link.So,if I understood the chart correctly,if I tried,as example,Strontium(-4.1),and Calcium(-3.8),I should get a cell with 7.9v potential?Next would be what happens with various electrolytes.Thanks for the fast replies!!</p>
<p>-4.1 - -3.8 = -4.1 + 3.8 = 0.3</p>
<p>I'm catching on :),Besides the links above(Thanks!),I found </p><p><a href="http://www.physics.usyd.edu.au/super/life_sciences/E/E5.pdf" rel="nofollow">http://www.physics.usyd.edu.au/super/life_sciences/E/E5.pdf</a></p>
<p>No, but it would increase the current you could draw.</p><p>For more voltage, you have to put cells in series.</p>
I didn't tried yet, I think it may not.
<p>What have you used it for and how long did the battery last in your application?</p>
Does it put off chlorine gas? Might want to put it in a well ventilated area
<p>How long does this produce energy until it is expended?</p>
<p>I wonder, what about capacity?</p>
<p>awesome !</p>
Awesome! Do you know what the capacity of this battery would be?
<p>Which of the chemicals described in the link below is in the "bleach powder" you have used? <a href="http://askville.amazon.com/diff-bet-chlorine-bleach-grocery-store--don-kinds/AnswerViewer.do?requestId=9255385" rel="nofollow">http://askville.amazon.com/diff-bet-chlorine-bleach-grocery-store--don-kinds/AnswerViewer.do?requestId=9255385</a></p>
<p>Series = Increased Voltage.</p><p>Parallel = Increased Amps.</p><p>It's a Fact.</p><p>Cool... will have to try it sometime... Thank you.</p>
en fait, la différence de potentiel, le voltage, est relatif à la pair de métaux choisie pour les électrode. C'est une question d'électro-négativité. <br><br>http://fr.m.wikipedia.org/wiki/%C3%89lectron%C3%A9gativit%C3%A9<br><br>Référez vous à l'échelle de Pauling.
<p>Wwell, I made some of them before with salt, vinegar, bleach and sulfur acid (separately) and it not worth. It can't do more than light up some LEDs :'(</p>
<p>What are you making copper electrod out of?</p>
Good! But how many Mah can produce?
<p>My son who is an electrician will be getting a link to this. Great job! </p>
It's really cool<br>We can connect the main points to a adapter than to phone.Will that charge phone<br>
I think it may not, because it not produces enough ohms and Mah to charge a phone.
<p>Don't you mean it has too high an internal resistance (to enable higher current flow) and has too little a capacity in mAh? Your comment doesn't make sense eletrically and gramaticly speaking.</p>
<p>It's possible - the easiest way is to use a module like <a href="http://www.ebay.co.uk/itm/7V-24V-to-5V-3A-DC-DC-Step-Down-Buck-Converter-Module-to-USB-Output-KIS3R33S-UK/400865889524?_trksid=p2047675.c100009.m1982&_trkparms=aid%3D222007%26algo%3DSIC.MBE%26ao%3D1%26asc%3D30259%26meid%3D006120da4ea741d9bdf80d3a84fd14f8%26pid%3D100009%26rk%3D3%26rkt%3D10%26sd%3D261582982584" rel="nofollow">this</a> which turns it into the requisite 5v. Note that the cells may not be able to supply enough power to charge a phone as it stands in this Instructable, so you might need to put more in parralel. </p>
It looks like you used powdered bleach - is that correct?
Yes, I am sure,If yo don't have the bleach, use acid solutions like salt water, lime juice etc.
This is super cool, you can probably power a good amount of LED lights with this.
