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collisions between the particles of gas and the container walls
No. The particles in a gas spread out and completely fill their entire container, regardless of the shape or volume of the container.
Pressure.
If the container is rigid, then its volume cannot change. However, if more gas particles are pushing on the walls, then it is the pressure that is changing.
Contact between the particles of a gas and walls of the container cause pressure in a closed container of gas.
Contact between the particles of a gas and walls of the container cause pressure in a closed container of gas.
the particles of gas bouncing into the walls of the container.
The particles will just move away from each other, to fill the larger container.
collisions between the particles of gas and the container walls
collisions between the particles of gas and the container walls
No. The particles in a gas spread out and completely fill their entire container, regardless of the shape or volume of the container.
The gas particles will spread out to encompass the entire volume of the container. The particles are constantly in motion and will run into the walls of the container creating pressure (basically). If heated, the particles will move faster, and slower if cooled.
Pressure.
The speed of the gas particles will increase as they are heated. That is why the pressure in a container increases. The particles are hitting the walls of the container with more force as they are heated.
In the gas phase, the particles spread out to completely fill their container.
If the container is rigid, then its volume cannot change. However, if more gas particles are pushing on the walls, then it is the pressure that is changing.
The greater the speed of gas particles in a container, the higher the overall average temperature and kinetic energy of the gas particles. And if volume was held constant, higher the pressure.