It rises, because you have packed more atoms into the same space.
The pressure inside of a container when nitrogen gas is added depends on:what the pressure was before the gas was addedhow big the container ishow much nitrogen gas is addedthe temperature of the gas before it is addedthe temperature of the container and its contents
In a closed system the pressure is directly proportional to the temperature (Gay-Lussac law).At higher temperature the volume tend to increase but in a container the volume is limited.
The pressure in a container is due to the particles of the gas hitting the inside walls of the container.
Even if the pressure inside a container is equal to the pressure outside a container, there is still pressure. It's like pushing a friend one way while he pushes you back. Neither of you may be moving, but you're still pushing. The sample of gas would exert exactly one atmosphere of pressure (or 100 kPa) on the container. The question then becomes whether the container can withstand that pressure.
Increasing the number of moles of gas, decreasing the volume of the container, or iIncreasing the temperature could cause a rigid container of gas to explode.
increases
The pressure inside of a container when nitrogen gas is added depends on:what the pressure was before the gas was addedhow big the container ishow much nitrogen gas is addedthe temperature of the gas before it is addedthe temperature of the container and its contents
increases......
Gas pressure decreases when cooling down a closed container.
Eventually it will explode because the heat causes the gas particles inside the container to accelerate and thus, create pressure by colliding with each other and the sides of the container. This pressure --> boom.
In a closed system the pressure is directly proportional to the temperature (Gay-Lussac law).At higher temperature the volume tend to increase but in a container the volume is limited.
They move Freely in the closed container.
The pressure in a container is due to the particles of the gas hitting the inside walls of the container.
The pressure inside the container will increase. Pressure (P) is force(F) divided by the area(A) it hits on. If you decrease the area, you increase the pressure.
false; it will increase; Boyle's law says P1V1/T1 = P2V2/T2
The pressure inside the container would decrease.
Even if the pressure inside a container is equal to the pressure outside a container, there is still pressure. It's like pushing a friend one way while he pushes you back. Neither of you may be moving, but you're still pushing. The sample of gas would exert exactly one atmosphere of pressure (or 100 kPa) on the container. The question then becomes whether the container can withstand that pressure.