Chemically, why does a can collapse with air pressure?
82527
This is not chemistry, but physics. I presume you are boiling water in a can, then sealing it and cooling it. There is then less pressure inside the can, since the water takes up less space than the water vapor. There is now more pressure outside the can than inside the can. You have unbalanced forces, and the can is unable to resist the pressure.\n\nThis can of course get far more complicated, and we can discuss the ductility of the can, and continuum mechanics of the can, and its chemistry, but I do not think you want anything that advanced. If you do, let me know.
676869
if you increase the pressure inside the vessel, which has an opening, vapour will immediately leave thru the opening keeping the pressure inside the same as outside.\n\nIf it was sealed and pressure increased inside, then u opened it, vapour would leave for the same reason to create a pressure equilibrium.\n\nThere is not formulae that i know of but pressure equilibrium is a known phenomenon
907233
With the air holes closed, there is a shortage of oxygen and the hydrocarbons in the gas do not burn completely. Some carbon is not burnt resulting in soot
898045
If you mean an aqueous solution of AN, then all it's gonna do it splatter, not explode.\n\nIf you mean you are trying to boil AN, not an aqueous solution, then you are correct, that is insane.\n\nUsually AN will decompose into nitrous oxide when heated.
310208
The balloon rises in atmosphere and remains intact till the point when its internal pressure is lower than the atmospheric pressure. At higher altitude where the atmospheric pressure is lower and the pressure inside the balloon is higher, it bursts as the rubber cannot withstand the internal pressure.
1168063
Air pressure.  It actually implodes not explodes.  There is no airpressure in the cargo holds at that height.  The key being that it was sealed.  Watch for shampoo bottles or anything like that.  I had a suitcase full of shampoo. :-(
126339
actually you should phrase it "why does pressure decrease when temperature is reduced?" because a rise or fall in temperature affects air pressure (not the other way around).  the higher temperature is, the faster molecules in the air are moving and therefore they increase the space they take up.  if temperature is lower, molecules move around less and require less space.
229524
Well. Okay its like this. Most times a chemical in a can is gas, but while its in the can its liquid. This is because of pressure. It pressurizes it to a point of where it would be if it were really cold. When something that is a gas at room temperature is cold, say below freezing, it would be liquid. When its compressed to a liqid state it is going to be cold. I hope this makes sense. Instant message me if it doesnt and ill explain more.
157020
It is Boyle's law & Charle's Law combined\nVolume of a gas is inversly propotional to Temprature & Pressure.\nOn Cooling can the Pressure & volume is decreased on can\nSince the outer layer of can feels pressure of air & it is more than inner pressure of can So it is crushed
93225
The gas is under pressure, so when you press the nozzel the liquid ....mmmmmm better a picture than words..\n\n http://www.aerosol.com/
811149
Gases are ultimately soluble in each other as noted by the atmosphere. If the pressure is increased, the molecules will get closer together.  But, the solubility stays the same.
260171
It isn't air! When water freezes all dissolved gases & other matter are not included!!! \n\nThe hydrogen bonds that form when water freezes creates an open structure. There is simply nothing in between those spaces.\n\nWe are talking about molecular structure, things at this level are so tiny that even thinking about what is in between is silly.\n\nIf there is anything between the spaces it is probably interstitial water molecules (those not hydrogen bonded inside the crystalline lattice structure - think of them as loose molecules of water).\n\nIce floats on water because it has expanded. That is all. Not because of what is in between the "spaces".\n\nSee, when you increase the surface area but have the same number of molecules present, you cause the object to become less dense. (it's less tightly packed...things that are tightly packed for their size are said to be more dense.)
814078
Pressure and volume are inverses of each other and therefore you can't in the first place say they are at constant pressure unless they were in the same container (When they do mix).. so when they are separated, you can't have the same pressure at different volumes. Though your experiment shows the achievement of equilibrium of high to low pressure, as the bigger one gets bigger (right?)...\n\nAnyways, finding an inexpensive experiment (on the web) is really difficult.  Dalton's law can be used as you probably know by collecting water over gases (which requires some lab equipment and some chemicals not readily available so to say) and also has an application in scuba diving.  I'll ask someone for you that I know... Can you give me 'till Monday or Tuesday to get a good answer for this or when does your presentation have to be done?
629212
The pressure between the inside of the can and the outside will equalize. It won't blow up in the sense of destroying the can. What might happen is that the metal near the puncture will tear a bit as the escaping gas rushes past it- in the same way a hole in a dam would 'grow' as water flows through it.\n\nProbably of more interest is that the escaping gas will be at a much, much colder temperature as it expands. This can lead to a surprising freezing effect at, on and near the can.\n\nIt is much more dangerous to heat a pressurized can without puncturing it. In this case, the can can fail as the pressure increases (due to the heating) and burst along a large seam instead of a small hole. Pieces of the can can be ejected quite powerfully in this scenario. The puncture scenario doesn't give you this effect at all.
169839
The chemical reaction to 'bond' two substances requires oxygen and the tube is "sealed" to keep most air out. It is not totally air tight however because if you let it go to long it will dry out in the tube. Also a little does stick to the inside but you never know it because you just assume the tube is empty and throw it out.
413571
Boyles law related the pressure and volume of a gas, as pressure goes up volume goes down and vice-versa. Charles law related temperature and volume, as temp goes up so does volume and vice versa.\n\nThe collapsing can demo really does not show either of these laws. If you boil a small amount of water in a can for a few minutes the water will turn to water vapor and expel most of the air out of the can. Then you need to invert the can and place it in cold water. This will seal the opening AND cause the water vapor in the can to condense. After the vapor condenses to liquid water, it takes up less space--- this decreases pressure inside the can, and higher air pressure outside the can crushes it. Not related to either law because they deal with gasses only, not gasses that change state to a liquid.
470974
The can and the air inside it expand. The can doesnt expand much, but the air does and a bunch of it flows out. When the can is placed in the cold water the can contracts really quickly and because there is less air pushing back on the walls it crunches up. There is nothing really big happening chemically.