Download
1 / 9
90 likes | 175 Views
Gas Laws By Maria Ward & Honorah Brown. Thirsty Candles.
E N D
In this experiment the water in the flask was heated and then a balloon was placed on the flask. As the temperature of the water decreased the gas inside the balloon lost volume and pressure. So the flask had less pressure inside the flask than outside the flask so the outside pressure forced the balloon inside the flask. Gases Don’t Suck!
In part C, the purpose of allowing the water to boil was to create a low pressure environment. Once the can with the boiled water was fully submerged into the pressure filled ice bath, the can collapsed in itself. There was more pressure in the ice bath than in the heated can so the cold water crushed the can trying to create equal pressure between the two atmospheres. Can you Take the Pressure?
In the medicine dropper, there was a small air bubble. As we squeezed on the bottle, the air bubble became larger and it sunk to the bottom of the bottle. This was able to happen because there was more pressure pushing down on the dropper. The medicine dropper is more dense than water, there for it floated, however, when pressure was added and the bubble inside of the dropper became larger the dropper became less dense and was able to sink to the bottom. The Cartesian Diver
The balloon with less volume remained upright after being poked with the pin. The second balloon which contained twice as much volume as the first balloon created a loud burst. This happened because there was more pressure occurring on the larger balloon. The higher the temperature the higher the pressure inside the balloon because the heat increased the volume which increased the pressure. • The law used in this experiment was Boyle’s law. Hot Spot
