Using Boyle's law and Charles law Gizmo. Think about a small helium tank that can fill 50 balloons what must be true about the helium in the tank compared to the helium in the balloons?
Based on Boyle's law and Charles' law, the following must be true about the helium in the tank compared to the helium in the balloons:
1. Volume: Boyle's law states that the pressure of a gas is inversely proportional to its volume, assuming constant temperature. Therefore, if the volume of the helium tank is smaller than the combined volume of the 50 balloons, then the helium in the tank must be under higher pressure.
2. Pressure: If the volume of the tank is constant and it is completely filled with helium, as more balloons are filled, the pressure inside the tank will decrease due to the increase in volume of the gas. Thus, the pressure of the helium in the balloons will be lower compared to the helium in the tank, assuming constant temperature.
3. Temperature: According to Charles' law, the volume of a gas is directly proportional to its temperature, assuming constant pressure. As the helium is released from the tank and fills the balloons, its volume will increase (assuming the temperature remains constant), which implies that the temperature of the gas in the balloons will be higher than the temperature of the gas in the tank.
Can you summarize that in a few sentences
Sure! In summary, if a small helium tank is used to fill 50 balloons:
1. The helium in the tank will be under higher pressure compared to the helium in the balloons, as the tank has a smaller volume.
2. As more balloons are filled, the pressure inside the tank decreases while the volume of the gas increases. Thus, the pressure of the helium in the balloons will be lower compared to the helium in the tank.
3. Assuming constant temperature, the volume of the gas in the balloons will increase as they are filled, indicating that the temperature of the gas in the balloons will be higher compared to the gas in the tank.