The molecules of the gas are in constant motion and their collisions with the sides of the container exerts a force which is felt as pressure.
Gas molecules collides with the container walls.
Kinetic theory explains the pressure that a gas exerts on the walls of its container. This describes elastic collisions between the atoms or molecules in the gas with the container's walls, which collectively exert a measureable pressure.
Heating a gas in a closed container would increase it's pressure. This would happen because when you heat the gas, the particles' kinetic energy increases, making them move faster, and more. They will hit the sides of the container and create pressure.
Cooling a pressurized container will cause the internal pressure to decrease.This works in reverse too. Depressurizing a pressurized container will lower the internal temperature (and by conduction, the temperature of the container itself). This is why ice often forms around propane gas cylinders after extended use.
If the lid was on the container all you would have to do is take the lid off so that the gas can escape. In other words, when the gas escapes, the amount of pressure is reduced (decreased). Certainly true if the gas pressure inside was originally higher than atmospheric pressure. Another way would be to cool it.
temperature is the average kinetic energy of the atoms of a gas. so with increased temperature the speed of the atoms of gas would increase. and since pressure is the collisions of said atoms on the side of a container; increased speed means more collisions of the particles and the side of the container increasing the pressure, and the same aplies for lowered temperature lower temp lower speed and less collions and less pressure.
A gas exerts pressure on the container because it is bouncing off the walls of the container at a certain force. The greater the force is the greater the pressure.
Kinetic theory explains the pressure that a gas exerts on the walls of its container. This describes elastic collisions between the atoms or molecules in the gas with the container's walls, which collectively exert a measureable pressure.
A simple way to think about it is: the pressure is the force per unit of area that a gas exerts on it's container caused by the molecules colliding with the container's walls. As the temperature increases, the molecules have more energy and collide with more force, so the pressure increases.
A gas.
The pressure will increase. if you have done solubility in chemistry it is like when you heat something to help it dissolve faster, this is because the heat gives the particles more energy to move around. Pressure is basically the force of the particles of the gas bumping against the container it is in, and as before with the dissolving, you are just giving more energy to the particles so they are bumping against the container with a greater force, therefore increasing the pressure
Contact between the particles of a gas and walls of the container cause pressure in a closed container of gas.
The pressure increases if the container gets smaller or the gas heats up. The pressure decreases if the container gets bigger or the gas cools off.
A gas consists of particles, which are either atoms or molecules, which all move randomly, and independently of each other. Every time a particle bounces off the wall of a container, it exerts some degree of pressure. The total of all the particles bouncing off the walls creates the pressure that we observe.
What causes the pressure exerted by gas molecules on their container? idk
The gaseous molecules are in continuous random motion and during their motion continuously strike the walls of container and exert the force on walls,the force per unit area is the pressure of the gas.
General Gas Law; PV=nRT just plug in your numbers and solve for 'n'
Greater pressure on a gas will compact the gas into a smaller volume. If the compressed gas is then warmed, it will try to expand, and the pressure the gas exerts on the container will increase. If the pressure becomes greater than the container can hold, the container will explode or split and the excess gas pressure released.