Basically what happens here is you empty the contents of an empty can of pop and fill it with some water. Bring the water to a boil and then place the can in a bucket of ice and the can will collapse because the pressure within the can is now much less than outside the can
I have two questions:
Would this be a good demonstration during an Ideal Gas Law/Van der Waals equation demonstration?
Why does the pressure decrease when some of the water in the can condenses from steam to liquid after being placed in the ice?
Is it because the volume of gas decreases so, therefore, the pressure decreaes?
My goal here is to perform a calculation showing how the Ideal Gas Law and van der Waals Equation will yield similar results at normal pressures and temperatures. So, if I were to be able to measure the volume of gas in the can after placing in ice condensed some of it into water, do you have to consider the water in the bottom of the can when finding your volume value? This may be a stupid question, so forgive me if it is.
The other one we were considering was taking a piece of filter paper and sliding it overtop a flash filled with water and then inverting the flask to demonstrate the pressure of the air acting upwards is holding the water.
The problem is relating these experiments to the van der Waals equation... any ideas?
Thanks in advance