DaWiz

I'm trying to build an alternator/generator that has the magnets rotating inside a coil of wire (or stator) to produce HIGH AMPS at LOW VOLTS. So what causes amps vs. volts: number of coils, magnetic field strength, rpm's, what?

wow...uh...Thanks John for your reply...however, I am running my batteries in parallel, not series...not that it really makes THAT much of a difference, I know. And to everyone else, YES! I KNOW THIS IS INEFFICIENT AND IMPRACTICAL! I just want to do it (who knows, maybe it'll eventually become practical with new technology). I'm in a friendly competition with a friend to see who can build a better small scale car and have always liked messing with H2...and my friend is using an electric motor setup (so that's why I'm not using a motor UC)

it's about a 2-3 pound car on a tiled hallway

I am running my batteries in parallel, but I'm just using Duracell coppertops. I don't know if it's ironic or not, but I have connected the five batteries' terminals with a thin piece of copper wire. The wire glowed red and the batteries got somewhat drained pretty quickly, but they still work. Also, I have acquired two transformers...one of which doesn't work and one of which I blew/shorted/melted/whatever. From pulsing my parallel setup, I have gotten readings off of my multimeter's scale: both in volts (AC exceeding 2000) and in amps (exceeding somewhere around 20). By the way, don't touch the wires on transformers....they hurt. Merged post follows: Consecutive posts mergedOkay, I took my transformer and dipped the output leads into a solution of sodium sulfate (these leads have the readings off the scale)...but the was little to no action as far as electrolysis is concerned? Any ideas on why it's not working?

I'm currently working on a project to make a small scale car, potentially Remote Controlled, that runs off Hydrogen that I produce by electrolysis ON THE CAR but I calculated that I need 2300 or so amps for peak performance (12000rpm). Here's my project idea (minus a few after-details): Take five 9V batteries and run them three step-up transformers each with a 20:1 coil ratio to theoretically yield 360000V...I have not done the calculation telling me how many amps that is, but I would think it would be quite a bit since I'm using copper wire (resistivity of 1.7x10^-8 ohm/m). Run the electricity into a sodium sulfate solution to put into a 4.4cc engine. This idea includes the fuel and exhaust to be a closed system (the "burned" water returns to be re-electrolyzed). Here's my calculation that leads me to need 2300 amps (12000rev/min) x (1 power stroke/2 rev) x (0.00017873mol gas/1 power stroke) x (2mol H2/3 mol gas) x (2 mol e-/1mol H2) x (6.022x10^23 e-/1mol e-) x (1.6x10^-19C/1e-) x (1 min/60sec)= 2296 C/sec = 2296 amperes This calculation uses a value derived from PV=nRT using 1atm and 300K Please let me know what you think. And I realize that I need to pulse my battery's DC current or otherwise convert it to AC for the transformer(s) to work.

I too tried electrolyzing water using AC current from the wall (carefully of course) using stainless steel (supposedly anyway--I used a paint scraper/putty knife that said "stainless steel). I did two trials. The first trial, I had the electrodes fairly well submerged in tap water, then pinched sodium sulfate salt into the water to increase the conductivity. After a few pinches, I had a nice stream of bubbles that evolved into a boiling frenzy. The second trial, I used an already prepared solution of sodium sulfate and barely had the electrodes submerged. The electrodes produced gas rapidly (not immensely rapid, though). In both cases, the water grew hot very quickly and the stainless steel rusted--suspension of iron oxide(s) in the water. So my question to anybody is do you think the 110V from the wall is the reason for the rapid rusting of my electrodes--i.e. would a lower voltage save my electrodes from putting out iron oxide suspension into the solution? (The problem with that is of course, less gas production b/c of less amps)

Magnesium Sulphate shouldn't produce sulfur dioxide...it should produce O2. Sulfate ions are actually difficult to oxidize, which is why it is a preferred anion to use in electrolysis: sulfuric acid is basically a standard, but sodium sulfate is a good alternative (I use it in my home experiments)