Gas pressure (in a container, for example) is due to the atoms or molecules bumping against the walls of a container. At absolute zero, the molecules have no internal energy, no speed - they won't move.
In practice, you can approach absolute zero, but you can never quite reach it.
If the gas were reduced to a state where the molecules ceased all motion, the pressure would be zero. In practical terms this is probably impossible.
Absolute Zero
An ideal gas would have zero volume at zero kelvin. This is an idealization, and it won't happen with a real gas. Also, real substances can't be cooled down to zero kelvin.
A barometric pressure of zero is a vacuum.
is motions of gas particles are related to the pressure exerted by the gas
Bjernkes force is exerted on a gas bubble when the gas bubble is in a liquid, is subjected to an acoustic pressure field, and undergoes volume pulsations. If the acoustic pressure gradient is not zero, it can couple with the bubble oscillation to produce a translational force on the bubble. This force is known as the primary Bjerknes force.
Absolute Zero
The pressure of a gas is exerted on the walls of its container by the movement of the molecules making up the gas. The higher the temperature, the faster the particles move, increasing the pressure exerted on the sides of the container. As the temperature decreases, the movement of the gas particles slows down, reducing the pressure. At absolute zero, the gas particles would be completely frozen so that no particles would be hitting the sides of the container and the pressure exerted by the gas would be zero. This is all theoretical since absolute zero cannot yet be reached, and gas would not actually be able to have a pressure of zero.
No.
Here's the ideal gas law: PV = nRT If T is zero, then PV must be zero; assuming the volume is nonzero, then for PV to be zero the pressure must be zero. However, this is only true for an ideal gas. For a real gas other factors come into play at low temperatures, and they begin to deviate from the ideal gas law. Also, all real gases liquify above absolute zero, and liquids don't obey the ideal gas law at all.
You can never get to -273 C or 0 Kelvin. But if you could, the pressure would be zero
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Zero. PV = nRT. T = 0, so nRT = 0, and thus PV must be zero also. Since we know the volume is not zero, the pressure must be zero.
Answer: computer says no?Answer: Also zero. This is hypothetical; an extrapolation. No real substance can be cooled all the way to zero Kelvin, and no gas would remain a gas at temperatures approaching that temperature.
Absolute zero is -273 degrees Celsius A: Actually, absolutely zero reflects a state in which an ideal gas exerts no pressure on its containment. As gas pressure come from movement, this temp depends on which components of the gas you're looking at: molecules, atoms, sub-atomic particles, etc. We have dropped electrons down as far as one picokelvin as of this writing. The actual number for ultimate zero, then, is not truly obtainable and is a theoretical constant.
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.
Boyle's law states that the volume of a gas is inversely proportional to its pressure if the temperature remains constant.
The way you state it, it is confusing. Absolute zero is a fixed temperature; therefore it doesn't increase or decrease.The volume of a gas will increase or decrease with pressure. The change in volume is such that if you extrapolate, it should theoretically have a volume of zero at approximately minus 273 degrees (Centigrade).The way you state it, it is confusing. Absolute zero is a fixed temperature; therefore it doesn't increase or decrease.The volume of a gas will increase or decrease with pressure. The change in volume is such that if you extrapolate, it should theoretically have a volume of zero at approximately minus 273 degrees (Centigrade).The way you state it, it is confusing. Absolute zero is a fixed temperature; therefore it doesn't increase or decrease.The volume of a gas will increase or decrease with pressure. The change in volume is such that if you extrapolate, it should theoretically have a volume of zero at approximately minus 273 degrees (Centigrade).The way you state it, it is confusing. Absolute zero is a fixed temperature; therefore it doesn't increase or decrease.The volume of a gas will increase or decrease with pressure. The change in volume is such that if you extrapolate, it should theoretically have a volume of zero at approximately minus 273 degrees (Centigrade).