Make Hydrogen Gas - Clean Burning, Inexpensive, Lighter Than Air!





Introduction: Make Hydrogen Gas - Clean Burning, Inexpensive, Lighter Than Air!

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This video demonstrates a purely chemical process to produce large quantities of hydrogen gas from common, inexpensive chemicals. Hydrogen is a highly esteemed alternative fuel candidate because its combustion with atmospheric oxygen results in only clean water vapor, rather than carbon compounds as is the case with most other fuels. It is less dense than air, which means that it can be used to lift objects into the sky.

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How does one dispose of the liquids in the flask and the bottle safely?

Yes, but it requires very dangerous amounts of electrical current to produce hydrogen as quickly as this. It also requires a more complicated setup to get hydrogen only, rather than a dangerously explosive mix of hydrogen and oxygen.

You still removing oxygen into there. Its 2 parts hydrogen 1 part oxygen you are producing . the only way to get pure hydrogen you need to use a separate cathode in a separate tube. I produce 2.5 lpm of oxyhydro in container for my Car. 12v 6 amps total. what your doing is just as dangerous since your using a corrosive chemical. I can do the same thing faster with a simple car batery.

You are incorrect. There is no oxygen involved with this reaction whatsoever.

2Al(s) + 6HCl(aq) --> 2AlCl3(aq) + 3H2(g)

I'm curious, how did you get 6HCl from a 300 mL aqueous solution?

for those of us without a chemistry degree, he's getting the hyrdogen from the acid, not the water. not sure why the water is needed exactly, but im sure there is a reason.

he said the acid mixture heats up. water is able to absorb heat very well

The water dilutes the acid so that the reaction is slowed to a controllable pace. It also helps to reduce bubble formation.

That's called a balanced chemical equation. It just tells you how many of one atom or molecule must react with how many of another to result in a whole number of products. If all you started with in the equation was:

Al + HCl --> ?

The products would have to be listed as fractional values, since there are not enough atoms given to allow you to form the complete molecules. Instead, the reactants are multiplied individually until they make a whole number of products, with no unreacted chemicals left over:

2Al + 6HCl --> 2AlCl3 + 3H2

This gives you a molar ratio that can be used to determine exactly how much aluminum or hydrochloric acid to react with a given amount of the other to have none wasted in the end. The equation tells you nothing about the quantity or concentration of chemicals that might be used to preform this reaction, it only gives a ratio, and shows all the chemicals involved.

If you wanted to do the math you could determine exactly how much HCl was in the 300 mL, and then from the equation calculate exactly how much aluminum would be needed to use it all, but I find it much easier to simply add the aluminum until it no longer reacts. Even if you did do the calculations, you could not add all the aluminum at once or it would react far too violently to be controlled, resulting in boiling acid spraying everywhere.