Gases
This is the hand warmer. The heat from our hand evaporates the ethanol in the bottle, increasing the pressure inside pushing it up the tube.
This is a video of Ramsey heating up the bottom of a can and then placing it in a bucket of cold water, crushing the can. The quick decrease in temperature made the pressure quickly go down, crushing the can.
When the inflated balloon was placed in the vacuum, many of us expected it to explode, but it only expanded. This was because the lack of pressure in the glass lid, allowed for the gas in the balloon to want to expand to fill the space.
This is what happens when a tea bag is lit on fire.
When the temperature inside the cup increases, it makes the pressure decrease. The pressure from the outside pushes the water up into the glass to fill the space.
This is a mini PTV stick. This was very helpful when going through examples and trying to figure out what was happening. For example when pressure increased, volume and temperature would go down.
During journey five, we learned about gases and their ideal states. An ideal gas is non-polar, preferably small, high temperature, and a low external pressure. We used many demos with gases to derive the formula PV=nRT, which is the Ideal Gas Law Equation. With that we were then able to solve real world problems and find out what the value of variables. The P, T, V stick was very helpful in conceptually figuring out what was going on in the problem and making sure we were right. It took me a couple of trys to get how to do the problems, but with more practice I continued to get better. I really enjoyed this unit, because we were able to take things that happen in the real world everyday and figure out why they happen.