Oxygen is a good thing. Oxygen is life. But if it were much more than one fifth of our air, we’d be in serious trouble. The other four fifths is nitrogen, an almost completely inert, obstructionist gas whose main effect is to get in the way of the oxygen, especially where flame is involved. For every bit of oxygen a fire consumes, it has to heat up and push away four times as much useless nitrogen. With pure oxygen, that damper is gone, and things that merely smolder in plain air go up like dry tinder. In 1967 three Apollo 1 astronauts died in a raging fire when Velcro lit up in their pure-oxygen pressurized space capsule.
Oxygen in gas form is used for welding and cutting: There’s no way to get a flame hot enough to melt steel using plain air. And in liquid form, oxygen is truly ferocious. For example, kerosene burning in air can power a camping lantern; kerosene burning with liquid oxygen powered the Saturn V moon rocket (yes, we made it to the moon on kerosene).
It’s not enough for space travel, but it’s possible to make small, controllable amounts of liquid oxygen using much more readily available liquid nitrogen. When a very thin aluminum container such as a beverage can is filled with boiling liquid nitrogen, dewdrops form on the outside and drip off the bottom. This is pure oxygen condensing out of the air (because the boiling point of oxygen is higher than that of nitrogen), just as water vapor condenses on a cold windowpane.
Achtung! Theodore Gray is a scientist trained in lab safety procedures. Do not attempt this experiment at home. Liquefied gases are dangerous and unpredictable, especially large quantities of liquid oxygen. For more information on Gray’s scientific pursuits, visit his website.
How can you be sure that the drops are oxygen and not just water? For one thing, if they were water they would freeze on the can. But the real test is to let the droplets fall onto some smoldering wood or paper. Believe me, there is no mistaking the effect of liquid oxygen on a fire.
This story has been updated. It was originally featured in the April 2008 issue of Popular Science magazine.