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What do you think will happen to the gas pressure as you make the container smaller?
The pressure will increase.
Use the Equation
P(1)V(1) = P(2)V(2)
Hence
P(2) = P(1)V(1)/V(2)
substituting some numbers.
P(2) = 5*10 / 2.5
P(2) = 50/2.5
P(2) = 20
So the pressure has increased four times, when the volume has been reduced to a quarter.
What else can I help you with?
Is the pressure inside the balloon equal to the atmospheric pressure?
Think about this: if the pressure WERE equal, what would happen in the instant when you open the neck of the balloon and whatever pressure is on the inside meets the pressure that is on the outside (atmospheric pressure)? In your experience, what DOES happen?
Does gas have a fixed shape and will it expand or shrink to any container?
No and yes. Well, it doesn't actually "shrink". "Compress" is a better word, because it takes 'pressure' ... you literally have to 'work' in the scientific sense to cram the same amount of gas into a smaller space. Just think of how hard it is to blow up a little balloon. You really have to do some pushing, but eventually you've got four or five lungfuls of air all into the little balloon. You can take any amount of gas, and if you push hard enough, you can stuff it into a small space. With any shape.
What if you put water in a dark colored container and a light color container which one will evaporate first?
The water in the dark-colored container will evaporate faster because dark colors absorb more heat from the surroundings, which speeds up the evaporation process. Light colors reflect more heat and therefore slow down the evaporation.
Which states identifies how the particles of gases affect one anothers motion?
The kinetic theory of gases identifies how gas particles affect each other's motion. It states that gas particles are in constant random motion, colliding with each other and the walls of their container. These collisions create pressure and affect the overall behavior of the gas.
What is a positive atmosphere container?
I think a vacuum flask wouldn't qualify. They probably refer to compressed gas cylinders such as breathing apparatus, oxygen cylinders, and the like. In which the gas pressure is above atmospheric.
If the air pressure inside a container were greater than the fluid pressure outside the container what would happen?
Okay i think i might know but i'm not sure but i think this can never happen because if it did the atmospheric pressure would crush us. our fluids in our bodies exert pressure on the atmospheric pressure(the same amount) and pretty much neutralize the effect!
If you were to transfer a liter of air into a 2-liter container how much of the 2-liter container would be filled?
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What causes the pressure that a gas exerts on the wall of its container?
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.
What will happen to the pressure inside a closed container of gas if more gas is added to the container?
It starts bubbling then it explodes. -I think it would just become more pressurized, it depends how pressurized it was before. But yes, it would explode if it had too much pressure.Yes, it could explode (depending on the type of container), but the main point is that the pressure would increase. Pressure is defined as the number and force of collisions between the particles and the wall of the container. If you're adding more gas to the container, then you are increasing the number of particles in one space; therefore, they will collide more often with the container.
What is the pressure caused by the collisions of particles in a water vapor with the walls of a container?
The pressure caused by the collisions of particles in a water vapor with the walls of a container is known as vapor pressure. It represents the equilibrium pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases (liquid or solid) in a closed system. At equilibrium, the rate of evaporation equals the rate of condensation, resulting in a constant pressure.
How can you make the pressure of air less than normal?
Well the easiest answer I can think of is to use the ideal gas equation and look at the terms and their effect on pressure. PV=nRT == P=(nrRT)/V, as can been seen from the equation: Pressure is directly proportional to Temperature and inversly proportional to Volume. So you trap air inside a fixed volume container. (Note: not every container will work. The walls of the container must be able to withstand the imbalance between the new inner air pressure and the atmospheric pressure.) Then simple cool the container. If you have gauge fixed to the rigid container (measuring the interior) you will see a drop in air pressure inside the container.
Why the pressure of a gas increases when it's temperature increases?
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.
How can you resist the pressure to drink alcohol?
just think of the hangovers and the all the things that can happen if you have alot of it.
What will happen when we start putting pressure and compress a gas enclosed in a cylinder and do you think increase and decrease in pressure can change the state of matter?
At high pressure the gas become a liquid.
Why do you think water from the different holes have different trajectories?
the trajectory of water is used as indicator of pressure. The longer the trajectory, the greater is the pressure at that point of the liquid column. Water pressure at any point in a closed container is dependent on the height of the liquid above it.
What is the unique quality of gases in relationship to volume?
A gas will expand to fill up any volume available to it. Think of rigid containers that will not change shape or volume. If you have 10 completely empty containers that can be connected. Inside each is a vacuum. Place some gas in the first container. It completely fills the container and creates some pressure. Connect a second container and some of the gas leaves the first container, but not all of the gas. The gas will completely fill both containers, but creating less pressure. Continue connecting containers, and the same appens every time. The gas completely fills every container that is connected and the pressure 'adjusts' on its own to reach a new equilibrium pressure.
What is the relationship of pressure and area?
THe larger the area the less pressure. The smaller the area the more pressure. THink of someone stepping on your foot, first with tennis shoes then with a spiky high heel. WHich would hurt more?
