GZunich said:Homework Statement
A tank is equally divided into two equal halves, one a vacuum and one filled with argon gas at 298K and 700 bar. The divider bursts and the gas equally disperses throughout the tank. What is the new T and P of the gas assuming argon is an ideal gas?
Homework Equations
PV=nRT P1V1/T1=P2V2/T2
The Attempt at a Solution
I assumed there was no temperature change which I am unsure of but using that logic, P=350 bar and T=298K
When a tank of gas is exposed to a vacuum, the gas particles will begin to expand and fill the empty space created by the vacuum. This process is known as diffusion, and it will continue until the pressure of the gas inside the tank is equal to the pressure of the vacuum outside.
No, it is not possible to completely remove all of the gas from a tank using a vacuum. This is because there will always be some gas particles that are stuck to the walls of the tank or are trapped in small crevices that cannot be reached by the vacuum.
The gas in a tank will not change state when exposed to a vacuum. However, as the gas particles expand to fill the empty space, the temperature and pressure of the gas may change. This can cause the gas to condense or evaporate, depending on the initial conditions of the gas.
It is generally safe to expose gas in a tank to a vacuum, as long as the tank is properly sealed and can withstand the pressure difference. However, if the tank is not designed to handle the pressure difference, it may rupture or implode.
The presence of gas in a tank will affect the vacuum pressure by reducing it. As the gas particles expand to fill the empty space, they will exert their own pressure, which will counteract the vacuum pressure. The higher the pressure of the gas in the tank, the less effective the vacuum will be in removing the gas.