I want to make my can explode. To what temperature so I have to heat it?
414884
Are you sure the unit is micropascal? I think there is an error in you units, its too small.\n3141.59 micropascal = 0.000000031 atmosphere\n\nPressure in ideal monoatomic gases is directly proportional to temperature, so: \nP1/T1=P2/T2\nT(ºK)=42,000*(177.94+273)/.000000031\n\nCheck the units and resolve it the same way.
1005734
That's a bit high...usually want to operate at about 40-45 C or less. Get yourself a better heat sink and cooling fan, and maybe a better cooled case.
1040977
It is done with steam. Just simple steam that you might get from a tea kettle. It doesn't have to be under pressure or any hotter than 212 deg F.
593326
Just use a garden hose.  Turn it on medium blast.  Works everytime.
737309
use a can of compressed air
934498
This is a three step problem.  Since you're losing heat temp is going down.  First calculate the amount of heat needed to go from 25.0 C to 0.00 C.\n\nq1 =  1 g X 4.18 J/gC X -25 = -104.5 J\n\nNow you have water at 0 C which needs to freeze.  You need to remove the heat of fusion to make ice.  deltaHf is -335.5 J/g.\n\nSo q = m X deltaHf = 1.0 g X 335.5 J/g = -335.5 J.\n\nNow we've used up 440 J so far, and the remaining 24 J will lower the temperature of our 1.0 gram of ice.\n\nThe heat capacity of ice is 2.1 J/gC and we'll need to solve for delta T.\n\n-24 J = 1.0 g X 2.1 J/gC X delta T\n\ndelta T = -24 J/ 2.1 JC= -11.4 C.\n\nSo the final state and temperature would be ice at - 11.4 C.\n\nSo the answer of -12 C should be correct with more care paid to significant figures and proper rounding.
1165181
It's been awhile since i've done this but i'll give it my best\n\nFirst off, the first energy you need to calculate is the energy needed to raise the temperature of ice to 0 degrees C. so...\n\n(12.37 g)(.48 cal/deg/g)(35 deg) = +207.816 cal\n\nWhen the ice changes to water you have a positive heat of fusion. So...\n\n(12.37 g)(80 cal/g) = 989.6 cal\n\nNext you have to raise the water temperature from 0 degrees C to 100 degrees C. So...\n\n(12.37 g)(1.0 cal/deg/g)(100 deg) = 1237 cal\n\nNext you have the positive heat of vaporization.\n\n(12.37 g)(540 cal/g) = 6679.9 cal\n\nNext once it is steam, you must raise the temperature from 100 degrees C to 146 degrees C. So...\n\n(12.37g)(.48 cal/deg/g)(46 deg) = 273.1296 cal.\n\nNow that you have the energy for each step add them together.\n\n207.816 + 989.6 + 1237 + 6679.9 + 273.1296 = 9387.45 cal\n\nI'm pretty confident in my breakdown but it defintely wouldn't hurt to have someone else check it
99103
throw it into space as high as you can, or just use that nitro
822974
You can grow a tree and fireproof it. Or find something with a pretty high combustion point and internalize the tree with. PERHAPS the tree won't burn. =)
725257
Well that's a good one though, I suppose you can't do that. What you think is simple is too complicated. We have a lot of problems maintaining the  temperature as a constant. You simply cant stabilize it. It will keep oscillating. You can still do it, but they'll be expensive and hard. It all depends on the surrounding temperature, where you put it, what the jugs are made up of(material) and so on.  But, you can maintain the temperature within a certain range. Contact your thermodynamics teacher for assistance.
858849
Easy. You heated the can, which means the air inside the can, including steam, was at a high temperature. That means it occupied more space. When you dunked it into cold water, the steam turned back into water, and the air in the can became more dense. The can crumpled because you basically created a vacuum effect. You decreased the volume suddenly by reducing the temperature.\n\nEnough?
747619
Does it have to be a material? the best solution for this would be to have 2 cans one just inside the other with a compleat vacume between them, as there is no air to transmit the heat between them the liquid inside wont change tempreture.\n\nthis is the principle of a thermos flask,\n\nif you need an actual material, somthing that would trap air to stop it from moving and spreading the heat such as glass fiber like you might have in your loft\n\nhope this helps
863405
To get the water in a microwave to go above 100C, you need to prevent it from boiling. The process of boiling takes up the heat required to raise its temperature.\n\nTo do this, you need distilled or deionized water (removing impurities/particles makes it harder for water to boil). When you microwave the water, it is possible to get it past 100C without causing the water to boil.\n\nBe careful when you do this however, the slightest agitation to the superheated water will cause it to EXPLODE and scald whatever it touches.
274231
It depends on the fuel type it is feeding off of. Many different things burn at different temperatures. Structure fires can burn at over 2000 (yes, two thousand) degrees Farenheight. Some metals can burn as hot as 4,000, to 5,000 degrees farenheight.
385620
It will not if the heat is moderate.  If the can is heated too much the increasing pressure will cause the can's valve to fail and some of the contents will be ejected from the can.  That which is ejected ould be expected to dry.
251863
At 20 degrees C, it's 0.6g/100mL. You can convert that to a Ksp.
549468
Add some baking soda first and then pour on some vinegar. You will observe some bubble forming and the bublbles will rise very quickly. If you want to make fire instead, add some glycerine to potassium permagnate. Be very careful if you want to do this.