Assuming constant amount of gas and temperature, pressure will increase as volume decreases. Conversely, pressure will decrease as volume increases.
If you squeeze on a filled balloon, the volume decreases. The pressure of the air on each square inch of the balloon increases, which causes it to eventually pop if the pressure gets too high.
Assuming constant amount of gas, a temperature change will already change the volume of the gas. As temperature rises, the gas expands, causing more pressure to be exerted on the balloon.
Assuming constant temperature, adding more gas also increases the volume and thus increases the pressure.
In a container, the pressure inside is exerted by the air molecules, striking the container's wall. When the air molecules increase in number, the pressure inside increases. This is because there are more collisions of molecules inside.
The kinetic theory states that gas pressure is the force exerted by gas molecules impacting on the sides of the container.
Collisions between particles of a gas and the walls of the container cause the pressure in a closed container of gas.
because your dumb
assuming it is an ideal gas: p=(nRT)/v=(3.2*.0821*373)/15 P=6.53 ATM
The pressure increases.
4.1 atm
As the volume is decreased, the same number of molecules of air have a smaller space to move freely in. The number of collisions of molecules of air with the walls of the container per unit time increases. Since pressure is the force exerted over an area, the pressure increases.
Vapor materials exert their pressure in just about every direction
'This is because the air particles are bumpinginto each other and the walls. When this happens it causes pressure on the walls because of the speed the air particles are moving
The fluids in your body exert pressure and prevent the atmospheric pressure from closing in. Fluids exert pressure on a container the particles collide with each other and the sides of the container.
Fluids are constantly trying to spread out, and that exerts pressure on the container you put it in.
To expand
The air molecules bouncing around off the inside of the tire. If you force something into a confined space that is usually allowed to be free it will exert pressure(Force) on th walls of it's container. An increase in tire temperature or friction will cause the air pressure to increase while colder temperatures will cause it to decrease.
assuming it is an ideal gas: p=(nRT)/v=(3.2*.0821*373)/15 P=6.53 ATM
As the molecules in the gas move, they collide with the container they are within. These collisions is what we call pressure.
Yes. Any sample of gas in a closed container will exert pressure on the container, as long as the temperature of the gas is above absolute zero. You can force the gas into a smaller volume by shrinking the container, but that action raises the temperature and pressure of the gas.
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.
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.
This is part of Boyle's Law.
The pressure increases.