The pressure is now higher.
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.
Reducing the volume will increase the pressure of the gas.
If the volume of a gas is reduced, the pressure increases. There is an inverse relatonship between the two variables.
The pressure will also fall. This may or may not be accompanied by condensation.
The pressure is now higher.
By reducing the pressure
You will recall from the Ideal Gas Laws that temperature, pressure, and volume are all connected in terms of the behavior of a gas (especially an ideal gas, but actual gas resembles ideal gas to a certain extent). So, if the gas is in a container of fixed volume, then reducing the temperature will correspondingly reduce the pressure.
The particles will move slower as energy is lost.
Yes it is possible. Boiling takes place when the saturated vapour pressure becomes equal to the surrounding pressure. So by reducing pressure over the surface of liquid even at 20 deg celsius it is possible to boil.
Pressure and Volume are indirectly propotional to each others. if you increase the Area the pressure will be decresed, and if you decrease the area of the applied pressure, the pressure will be automatically increased, Hence. Pressure if Indirectly propotional to Area.
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.
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.
hi bye bye
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.
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.
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.
Volume and pressure vary indirectly, which means that when one goes up, the other goes down. If the pressure goes up, the volume goes down. If the volume goes up, the pressure goes down.Mathematically:P1V1 = P2V2The left side represents the beginning conditions, and the right side represents the pressure and temperature that have changed. Note that this formula assumes constant mass and temperature.
By reducing the pressure
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.
240 Assuming ideal gas behavior, doubling the pressure means reducing the volume by a factor of 2.
Yes.
Usually by adding heat and/or reducing pressure.