In that case, the pressure increases. Specifically, the pressure will be proportional to the absolute temperature.
Given that the container is "rigid" the size of the container holding the gas cannot change. Since the volume of the container remains constant, so too does the volume of the gas. The pressure however will increase.
When heated, temperature increases. You may have already guessed that. Most substances, but not all, increase in volume as the temperature increases at constant pressure. The pressure would remain the same if the fluid was in an open container.
As you heat, volume would normally increase, but because this cannot happen in a closed system, pressure will increase inside the container
The pressure is higher.
It doesn't unless it is constrained in a constant volume container. When in a container, as the air is heated its molecules vibrate more and take up more volume - as the volume of the container is fixed then Charles's law applies and the pressure goes up.
If you decrease the volume of the container, the pressure rises, and vice versa.
In a sealed container the volume remain the same and the pressure increase.
If the volume of a container of air is reduced by one half the partial pressure of the oxygen with in the container will be doubled. If the volume of a container of gas is reduced, the pressure inside the container will increase.
Pressure increases as volume increases, granted the container stays the same.
If volume goes down the pressure goes up
Assuming you haven't put any more gas in the container, the pressure will go down. Usually, the reason the volume of the container gets larger is that you put more gas in the container and the gas pressure in the container seeks to equalize with the pressure outside it.
This relies on 3 things. The Pressure, volume and temperature of a Gas is all related. If the pressure is kept the same and temperature increased. The Volume (of the container) must be increased. If the Volume (of the container) is kept constant and temperature is increased the Pressure will increase. A rough idea of what will happen can be worked out by, pV=cT Where p is the pressure, V is the volume of the container, c is a constant, T is the temperature.
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.
In a small volume container the pressure is higher.
If the volume stays the same, the pressure will decrease.
Depends on the container of the "air particles" and what you mean by "what happens." If it is inside a container that can not expand, then the pressure increases. If it is inside a container that can expand (or is just atmospheric air) then the volume increases. (Pressure * Volume = n * R * change in temperature) On the atomic level, the atoms or molecules (depending on the gas) begin to move more quickly as their kinetic energy increases.
If you have a fixed volume container and pump more air into it, the volume will remain the same as you increase the pressure. However if you have a variable volume, sealed container and you reduce the volume of the container (say by sliding a piston down it) then as the volume decreases, the pressure will go up.
As volume decreases, pressure decreases as well.
If the contents in the container are gaseous, then the pressure will increase as temperature increases. The pressure will decrease as temperature decreases.
If you increase the volume of the container, and not the gas itself, then the pressure decreases. If you increase the volume of the gas, and not the container, then the pressure increases.
If the gas is in an inclosed container, the pressure will increase. If it is free to expand, it will have a greater volume.
Assuming the volume is kept constant, the pressure will also decrease in this case.