Something similar happened to me

CO2 is also quite heavy, which makes it floating capabilities worse

depends on the availibility

if you have enough carbonate and a minute amount of HCl it‘ll be fine bc it first generates hydrogencarbonate. Also I feel like you would start to see small bubbles accumulating at the side of the gas wash bottle bc if the CO2 in solution

Since the gallium removed the oxide layer and exposes fresh aluminium which does react with water.mixing gallium and aluminium is producing a rxn the same as aluminium mercury amalgam.

+Chad Howarth It may have burned slowly because it had to take the time to escape the bag and mix with the air before it could combust. If it were already mixed with the air in the bag it would probably burned much faster.

He made a pretty good job at letting the whole apparatus filling with hydrogen, so there was no explosion because it requires oxygen ! and the bag did not contained enough to allow an explosion

+Chad Howarth It could be all of those things. If I had an experiment that needed pure, dry hydrogen, I would certainly have used NaOH in the bottle. It's just expensive and I was looking for a quick solution for the demo. The problem with smart subscribers is that you can't get away with anything! :D

+Doug's Lab Isnt it better to just skip the acid, and react NaOH(aq) + Al to make hydrogen gas?

Doug's Lab come on now...NaOH isn't _that_ expensive

It's too violent usually and you have to have cooling baths and all that

@@EdwardTriesToScience yeah I know that, sometimes the reaction gets out of hand , but it's an easy source to produce any hydrogen gas. :))

@@Prchemist06 Yeah I actually used that reaction alot before I found out I could get HCl for wayyyyyy cheaper, the only problem (other than runaway reactions) was the hydroxide solution getting hot enough for long enough that it'd start to etch the glass, otherwise its a nice reaction

@@EdwardTriesToScience yeah it's an annoying property of NaOH to etch glass.

Which might explain the shitty silent hardly did anything rxn with the flame when it was lit on fire.sodium hydroxide is definitely the best thing to use.u r right carbonates will contaminate the gas stream with CO2.also I am curious to see if the H2 contains hcl. My experience tells me more than one wash bottle would be needed.i bet if U held a piece of pH paper against the gas outlet it would indicate that it's heavily acidic still. I think hcl +aluminium is the worst way to produce CLEAN hydrogen.

The set up for that process is as follows: Take a container that can fit a test tube or something similar in it. Fill it with water and an electrolyte. Put a a test tube or similar container with the hole towards the ground into the larger container. Make sure the test tube is filled with water completely so there is no air in it. Place your electrodes so that the electrode that produces hydrogen which I believe is the negative one (not sure) is inside of the upside down test tube. Place the other electrode in and turn on power. Oxygen will be made but will dissipate into the air but hydrogen will displace the water in the test tube. Your hydrogen will be contaminated with a little bit of water vapor. With this set up it's basically impossible to avoid that just because of vapor pressures and such.

+Elisabeth Esther Mostly the hardware store and eBay.

@@DougsLab can I get the contact number

Mg metal and h2so4 leaving Epson salts or aluminium and sodium hydroxide.

Dry MgSO4 is cheap..bake Epsom salt at 300°C for two hours on a sheet just a few mm deep. Weigh before and after, it is over half water.

no

phosphorous is not a metal

Ag(s) + HNO3 (aq) = H2(g) + AgNO3 (aq). NO2 and N2O4 are produced from the nitric acid breaking down.

+Clyde Wary Excellent observation! I totally missed that when I was preparing the lecture segment. I have added an annotation to correct it.

+Doug's Lab Great! I sent you a message, before I found out you made the necessary correction. Thanks :)

also, I am surprised Zn isn't on the list; and please review that chemical equation (Al+HCl)

Actually, the NaOH is just a catalyst. Aluminum oxide and hydroxide are quite insoluble in water. NaOH breaks the oxide/hydroxide layer, allowing the water to react with the metal. Look up the rocket propellant called AlICE. Also used in slurry blasting agents

@@keithjurena9319 Oh, thanks for the insight. Sounds like I've been wasting quite a bit of NaOH in the past then lol.

On the other hand, if you actualky write down the reaction between Al, H20 and NaOH, it looks like the Na is actually used up in the reaction, not recovered like a catalyst would be. It also makes a difference how much water is available since you'll either make anhydrous or hydrated aluminum hydroxide.

+bdot02 This is just one method among many. But it's the "classic" method that everyone learns in a basic chem class. Electrolysis is certainly cheaper. And here's another one... Several decades ago, I saw an ad in a surplus catalog for weather balloons. The balloons included cannisters of CaH2, which when added to H2O, produced the H2 for filling the balloons.

+Constantino Fine Art SHHH!!!! You're not supposed to notice that. :) I really need a gas washing bottle with a fritted sparging tube.

I know from experience that heaps of HCl gas is given off as well in this rxn and I'm wondering if U checked whether you're hydrogen still had hcl in it? Like did U hold a piece of pH paper against the gas stream? I'm not convinced that one bubbler is enough.personally I'd use multiple wash bottles.