First, hydrogen peroxide is: H-O-O-H. Remember that list of bond dissociation energies that I posted? Take a look at the H-O bond strength and then the O-O bond strength. Which one would you expect to be cleaved first? Yeah, the O-O single bond. I think it's like 35 kcal/mol or something like that. It's quite weak.
Second, your tanning booth experiment: pure H2
would most likely explode. It's not that stable in highly concentrated form as it is, slowly decomposing at room temperature (mostly due to impurities), but in a tanning booth, it'd probably explode. If not, you'd at least have a lot of effervescent decomposition.
Next, organic peroxides, in almost every case (I say almost every because although I can't think of an example where this is not a case, I'm sure that AWK will come along and prove me wrong) are dangerous explosives. Unless you are using hydrogen peroxide, alkali peroxides, ethers, or some fancy organic molecules, you're not that likely to form them. It's a problem in organic chemistry because we have to evaporate things to dryness and if you've got peroxides in the solution, they don't like the heat of a rotovap bath.
Even in solution, peroxides can be unstable, but are generally more stable when in solution.
The military generally won't touch peroxides because they are way too sensitive. Tiny amounts of friction, flame, shock, heat, or impact can cause them to detonate. Terrorists like to use them because they are easy to form if you have the right chemicals, but those idiots don't care if they lose a few people making destructive devices. Hell, they tend to blow themselves up most of the time anyway. We used to make very tiny quantities of organic peroxides for class demonstrations back where I did undergrad, and they were pretty impressive. We'd have only about 0.07g of peroxide, less than the size of a crushed up aspirin, and we'd hit it with a hammer, pretty much just letting the hammer drop on the pile, and it would detonate. The students loved it, but we were careful to be safe about it all. The remainder of what was left on the filter paper we'd burn off, as it wasn't enough to detonate, and we'd get a resultant fireball. My avatar is a picture of one of our burn-offs of a nearly microscopic amount of peroxide. We weighed that particular sample, and it's 0.001g. That's 1 mg. Nothing. You could barely see any white dusting at all on the filter paper, and when we brought a glowing wooden splint up to it, we got a fireball about 10" in diameter. That is dangerous, I don't care who you are. So, bottom line: if you make organic peroxides, in whatever capacity, you're asking for a whole lot more trouble than you bargained for, even if you think that you're prepared for anything.