# How difficult is it to produce diatomic hydrogen?

Just to preface this, I have a very basic understanding of chemistry, so forgive me if what I'm asking is super basic.

How difficult is it to produce diatomic hydrogen? I've been doing some reading on the internet about diatomic hydrogen and a fair amount of the stuff I've come across are health articles relating to the benefits of drinking hydrogen rich water, so I assume that it's not terribly difficult to come across.

• There are several easy ways to produce pure hydrogen, e.g. electrolysis of water. However, hydrogen is a gas at room temperature, so I would seriously doubt that there actually is something like hydrogen enriched water. I would further doubt that if such a thing existed, it would have no health benefit. – Martin - マーチン Feb 10 '16 at 7:40
• There is a NIH study on hydrogen water so it isn't totally poppycock. ncbi.nlm.nih.gov/pmc/articles/PMC2831093 – MaxW Feb 10 '16 at 21:34

The simplest way to do this with household means is probably to use acetic acid concentrate (the stronger the better) and zinc powder. (Solid zinc works but much slower.) The reaction may be sluggish; if that is the case, very carefully and slowly heat the acetic acid. Capture the hydrogen in some glass, cup or test tube held upside down (hydrogen is the least dense gas with each molecule only weighing $2~\mathrm{u}$ (atomic mass units) so it will always rise).
If you have collected some amounts of hydrogen gas you can proove its presence. This was a common experiment in my high school chemistry courses so I’m going to tell you how to do it. However, exercise caution! If you didn’t do this at school yourself or didn’t watch someone do it before, I would advise you to not attempt it. Only do this with very small amounts of hydrogen, no more than a test tube of $2~\mathrm{cm}$ diameter. Make sure the test tube is full (by collecting enough hydrogen). Carefully bring the opening towards a candle flame. Do not use a pocket lighter where your thumb is right next to the flame for safety reasons. The hydrogen should burn with a faint ‘pop’ creating water. Considering how slurrish the reaction of zinc and acetic acid probably is, it may be too slow to actually collect enough hydrogen. Don’t attempt the burning if that is the case.
The reason for being cautious is the following: $2\,:\,1$ mixtures of hydrogen and oxygen are explosive. And with explosive I mean that they give a very loud bang. Luckily, air is mainly nitrogen so the probability of accidentally creating an explosive mixture is rather low. However, if you did, you will regret it.