why gas can be compressed easily?
97649
I don't like the term "easily", because that's vague. Gases can be compressed, as people have noted, because the space between gas molecules is large but unoccupied. However, you do have to perform work in order to compress a gas (thereby using energy).
985658
So living things can breath. Without air pressure we would not be able to breath.The air is thinner up in the atmosphere.Down here the air is Thicker and more dense then up there that's how we can live,with air pressure.With too much pressure or to little we could die.With too much pressure we could implode. Or too little pressure we could explode (I don't know how that would be possible but I think it's right) .That sounds funny that we would explode with too little
894173
Gases disperse to fill whatever container they occupy.   Gases are composed of matter and thus occupy space.  Since no two objects of matter can occupy the same space at the same time and a gas expands to occupy a given space a force(pressure) exist.  As the temperature increases the pressure increases because you are adding energy to the system.
499971
When gas is compressed in a thermally insulated vessel the gas is heated.\n\nWhen pressure increases temperature increases.\n\nSimilarly if the gas is expanded in a thermally insulated vessel the gas is cooled.\n\nWhen the pressure decreases the temperature decreases. \n\nNear earth’s surface, the atmospheric pressure is very high.\n\nAt a height of 30km from the surface, the pressure of air is almost zero.\n\nThough the hot air goes up; as it goes up the pressure decreases and volume increases (density decreases) and as per the  gas equation the temperature decreases.
383470
Personally I use C02, but a Nitrogen tank is EXPENSIVE, but it gives so much more added volcity, Compressed air is simmilar to C02, expept you can fill it yourself if you have a special tank and compresser.
1175149
A solid, unlike a liquid or a gas, does not take the shape of its container.\nPour some water into a glass and the water takes on the shape of the glass, pour this water onto the floor and now the water has an entirely different shape.  The same goes for gasses.  However, put some solid object in a glass, on the floor, ..., and it still has the same shape.\n\nBoth solids and liquids have definite volumes, unlike gasses.  Solids and liquids are considered "incompressible".  No matter how much you squeeze them, they retain their volume.  Gasses however can be compressed/expanded depending on the force acting on them.
316023
intermolecular polarity and the fact that fluids dont compress the way gases do?
511368
It is possible to compress all gases, liquids, and solids. It is simply a fact that liquids take much more pressure than gases, and solids much more than liquid. The reason for this is the spacing between atoms. In gases, there is a lot of spaces between atoms, so it only takes a little pressure to close these spaces, and hence pressurise the gas. Obviously, with liquids such as water, the gaps are FAR smaller, so there is much less room for the atoms to move into, so it needs a MUCH, much higher force to pressurize it.\n\nYou would also need to take temperature into account, because as the temperature of a gas/liquid/solid increases so does the size of the spaces between atoms, and thus a lower force is needed to pressurize the substance.\n\nSo the answer to your question is that yes, there IS a presuure at which it would be possible to pressurize water, but it is going to be extremely high, and will vary depending on several other factors
882307
Sorry but only the first answer was close.  The air inside the baloon is compressed, because of its containmentt inside the stressed rubber.  (You need to blow to fill a baloon).  When the rubber is split, the air expands rapidly to equal the surrounding pressure.  This rapid expansion propogates outward, causing tha bang
917314
A real gas is a form of matter that will conform to the sides of its container.  As it is compressed its temperature increases.  It is the only form of matter than can be compressed at all.  Gas is the least organized form of matter.
669055
A) Entropy causes gases to evenly fill up a defined space, meaning in the absence of other influences, you get equal pressure (concentration) everywhere. Diffusion, or spreading of the gas molecules ensures that. This is why a bag of garbage will eventually stink up a whole room and not just part of it.\n\nB) Think of a balloon. Unless some force is exerted on the baloon form the inside, the rubber would naturally contract to its uninflated state. Gas particles bouncing around exert a force on the container wall, much like firing tennis balls against something in order to stop it from approaching you.
719883
you are using les power therefore less gas is required
186473
Compressed gas supply company.
552949
Use of pressurized gases to do work.\n\nFor more info, see this:\nhttp://en.wikipedia.org/wiki/Pneumatic
315960
Properties of Gases \n\n1.  Indefinite shape -- you can squash an air-filled  balloon to make circus animals\n2.  May expand -- balloons get bigger when temperature gets warmer\n3.  May compress -- can put lots of air into a car tire\n4.  Have low densities -- balloons filled with air will float on water\n5.  Diffuse uniformly -- put a pizza on the front seat of the car and the people in the back seat get hungry pretty quickly -- that pizza vapors travel to fill the car! \n\n11.2  Atmospheric Pressure \n\nEven though we can't see the air around us, we know it's there and those molecules bouncing around exert a force on our bodies.  Fortunately, the force is the same on all sides of us, so it equalizes out and we don't notice that we're pushing against the air as we move our bodies. \n\nWe use a barometer to measure pressure.  We can use lots of different units depending on the system we're using.  Normal atmospheric pressure at sea level is defined as "1 atmosphere of pressure";  we call this by the special name "standard pressure".  The equivalent measures in other  units for standard pressure are given in table 11.1;  when we talk about standard pressure in this course we will use units of atmospheres, mm Hg and torr.  You're probably familiar with the weatherperson talking about pressure in inches of Hg.  If you use 2.54 cm = 1 inch, you can do the conversion from inches of Hg to cm and then on to mm of Hg.  There's no magic here, it's just a metric/English conversion example. \n\nYou may be curious about how a barometer works.  Here's my interpretation.... \n\nLet's start with the diagram on page 295 which is a representation for the workings of a barometer. It helps to talk about how this setup is put together. One would hold the tube "right side up", that is, like a test tube and fill it "to the brim" with mercury. One then inverts the tube in a pool of mercury (taking appropriate safety precautions). Immediately some of the mercury will flow out of the tube. How much flows out depends on how much pressure the atmosphere exerts on the pool of mercury. If the atmospheric pressure is higher, there is more pressure on the pool of mercury and the material in the tube stays at a higher level. If the atmospheric pressure is lower on a given day, more mercury is allowed to flow out of the tube. If the atmospheric pressure increases again, more mercury is pushed pack up into the tube. It is important to recognize that a virtual vacuum (except for a few stray mercury molecules) exists above the liquid in the tube which exerts no pressure (has no influence) on the height of the material in the tube. The only influence on the height of the material, is the air pressure on the puddle of mercury at the bottom.\n\nThe number the weatherperson gives is the height of the column measured in inches or mm (of mercury). We use mercury because it is so dense. If we were to use a water column instead (mercury is 13+ times as dense as water), the column would have to be 13+ times as high.  \n\n  Do example exercise  11.1 and the self test.  You can make up unit factors using any pair of these units to do homework exercises 5 and 7. \n\n11.3  Variables affecting Gas Pressure \n\nThink of gas pressure as the effect of molecules hitting the walls of a container.  When the molecules hit harder, the pressure is increased.  The tire pressure in your car can be affected by 3 things:\n \n  \n\nVariable What we measure Predicted effect on pressure of the gas Why? Also true (follows logically); complete with increase or decrease \nvolume of the container how much air the tire can contain increase volume, decrease pressure more space for the molecules to move around, so don't hit walls of container so hard decrease pressure, (       ) volume \ntemperature of the gas temperature of the air in the tire increase temperature, increase pressure molecules moving faster, so hit
1102426
BY PRESSURIZING IT AT HIGH PRESSURE & COOLING THE GAS SIMULTANEOUSLY IN LOW PRESSURE
30270
In general, a gas turns into a liquid by cooling it.