Explain Why the pressure of a gas in a nitrogen container falls continuously when the gas is continuously taken away while the pressure of a gas in a chlorine container remains constant until nearly all the gas is withdrawn
depends on temperature
BUT
I suspect that there is liquid chlorine in the bottle. If so then the pressure remains at the vapor pressure of Chlorine until it is evaporated.
The N2 is all gas in there until you get down to liquid air temperature so it follows gas laws.
The pressure of a gas in a container is determined by the number of gas particles colliding with the walls of the container. When gas is continuously taken away from the container, the number of gas particles inside decreases. As a result, fewer gas particles collide with the walls, leading to a decrease in the pressure.
In the case of a nitrogen container, as the gas is continuously taken away, the number of nitrogen gas particles inside the container decreases. With fewer particles colliding with the walls, the pressure of the gas gradually decreases over time.
On the other hand, for a chlorine container, the pressure remains constant until nearly all the gas is withdrawn. This is because chlorine gas consists of diatomic molecules (Cl2), meaning two chlorine atoms are chemically bonded together. Since the gas is withdrawn without breaking the chemical bonds, the number of chlorine molecules remains constant even as the gas is removed. Hence, the number of particles colliding with the walls of the container remains the same, resulting in a constant pressure until almost all of the chlorine gas is withdrawn. Only at this point, when there are very few chlorine molecules left, will the pressure start to decrease.
In summary, the difference in behavior between the two gases is due to the presence of individual gas particles (nitrogen) versus chemically bonded molecules (chlorine) in their respective containers, resulting in differences in how the pressure changes as the gas is withdrawn.