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Answered 2010-09-29 02:07:00

At a constant temperature, the volume and the pressure are inversely proportional, that it, the greater the volume, the lesser the pressure on the gas, and viceversa.


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If the volume of a gas is reduced, the pressure increases. There is an inverse relatonship between the two variables.

That depends on the experimental conditions.In a situation of constant pressure, the density will also be constant.In a situation of constant volume, reducing the amount of gas will reduce both pressure and density.

Reducing the temperature would be one way, or reducing the pressure.

If you reduce the air pressure you make it 'easier' for water particles to become gaseous as there are fewer gas particles colliding with them on the surface, reducing their energy. Without this interference they gain enough energy to become a gas at a lower temperature.The converse is also true. If you boil a liquid under pressure there are so many gaseous particles colliding with the surface of the liquid, reducing the liquid particles chance of 'escape'. This means a pressurised liquid boils at a higher temperature. It's this feature that is used in pressure cookers to cook things quickly, because they reach a higher temperature.

240 Assuming ideal gas behavior, doubling the pressure means reducing the volume by a factor of 2.

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.

Charles's Law states: At constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its temperature (in Kelvin) increases or decreases. Volume /temperature = K (constant) Boyle's Law states: Boyle's law states that at constant temperature, the absolute pressure and the volume of a gas are inversely proportional. Pressure Volume= K (constant) It can also be stated this way: Forcing the volume V of a fixed quantity of gas to increase, while keeping the gas at the initially measured temperature, the pressure P must decrease proportionally. Conversely, reducing the volume of the gas increases the pressure. These are gas Laws scuba divers must know.

You can reduce the pressure of a gas by any of the following:* Reducing the amount of gas (letting some gas escape) * Reducing the temperature * Increasing the volume

it is because as temperature increases, the particles in the water surface move further apart thus reducing the surface tension

The weight of the air The distance between particles of a gas determines the pressure. The distance can be decreased and the pressure therefore increased by either increasing the amount of particles of gas in the container, or by reducing the size of the container.

Usually by adding heat and/or reducing pressure.

Reducing the volume of a gas does what to its pressure?

BOYEL'S LAWAt constant temperature, the volume of a fixed amount of gas is inversely proportional to pressure.The mathematical equation for Boyle's law is:where:P denotes the pressure of the system.Vdenotes the volume of the gas.k is a constant value representative of the pressure and volume of the system.{So long as temperature remains constant the same amount of energy given to the system persists throughout its operation and therefore, theoretically, the value of k will remain constant.} However, due to the derivation of pressure as perpendicular applied force and the probabilistic likelihood of collisions with other particles through collision theory, the application of force to a surface may not be infinitely constant for such values of k, but will have a limit when differentiating such values over a given time.Forcing the volume V of the fixed quantity of gas to increase, keeping the gas at the initially measured temperature, the pressure p must decrease proportionally. Conversely, reducing the volume of the gas increases the pressure.Boyle's law is used to predict the result of introducing a change, in volume and pressure only, to the initial state of a fixed quantity of gas. The before and after volumes and pressures of the fixed amount of gas, where the before and after temperatures are the same (heating or cooling will be required to meet this condition), are related by the equation:

Reducing the volume will increase the pressure of the gas.

Solidification of water depends on both temperature and pressure. Experimental phase diagrams are available in any text book on the subject. For a given pressure (in most circumstances) once the temperature is below the solidification point, reducing the temperature generally will not change its state.

this is somewhat a guess but somehow reducing the pressure will cause it to boil at a lower temperature because the molecules will be closer together and not need as much energy to collide... this is somewhat a guess but somehow reducing the pressure will cause it to boil at a lower temperature because the molecules will be closer together and not need as much energy to collide...

Any of the following: increasing the amount of gas; increasing the temperature; reducing the volume.

The easiest way is to install two pressure gauges (If reducing pressure) either side of the reducing valve, you will then have indication of upstream pressure and down stream pressure, of which you can adjust to suit you process.

On decreasing kinetic energy, particles will move at a lower speed than before. The rate of collision will also reduce. Reducing the temperature will decrease kinetic energy.

Prevents particles from aggregating together,reducing agent homogenously incorporated insolution allows for better 'capping' of particles, not allowing them to grow and producing monodispered particles.

Some methods are:- increasing the temperature- stirring- if the solute is a solid, reducing the grain sizes- increasing the pressure

For an "idea" gas there is a special equation that describes what happens when gas particles slow down. PV=NRT Rougly, Pressure times Volume equals Number of "Moles" (an quantity the represents the number of atoms in the gass) times a constant R times the temperature. So if gas particles slow down it means they their tempure (T) has gone down. This means that either the pressure (P) or the volume (V) must go down, or both. You can demonstrate this by putting an inflated balloon in the freeze for awhile. A balloon of the same size left out of the freezer will retain it's size but the chilled balloon will be noticable smaller. This is because the air has gas particles that have slow down, reducing the pressure and therefore shrinking the volume.

pressure relief valve relief the excess pressure which is developed in the syatem, while pressure reducing valve reduces the pressure and supply it to the system.

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