# Does gas spread out equally everywhere?

Gases can fill a container of any size or shape. It doesn't even matter how big the container is. The molecules still spread out to fill the whole space equally. That is one of their physical characteristics.

If a fixed quantity of gas is let out in a limited space, will it spread out equally and maintain a fixed gas distribution throughout the space?

Or, does it go where the gravitational pull is maximum? And what factors affect the distribution of gas in a given area?

• I'd also like to know, more practically, what happens if you let out a bit of gas from a tank on the ISS, ignoring rocket effects?
– user12029
Commented Aug 10, 2013 at 9:31
• @NeuroFuzzy - the ISS has fans a-plenty. Commented Aug 10, 2013 at 9:57
• @DeerHunter, huh?
– user12029
Commented Aug 10, 2013 at 10:30
• Not just gravity, but any (Newtonian) force . Commented Aug 10, 2013 at 11:35

Yes, without gravity, the gas fill out the space evenly so you can get uniform distribution of gas. Certainly, it only occurs at thermodynamic equilibrium, that is, if you wait for a long time.

With gravity, the density would be higher at location of lower gravitational potential. If we can treat the gas as ideal gas, then each gas molecule is independent with each other and the distribution will be following the Boltzmann distribution $e^{-E/k_BT}$.

Near the surface of the Earth, the energy is roughly given by $E=mgh$, therefore the higher from the ground, the lower the density and it decreases exponentially. Real situation are more complicated as the molecule can absorb light energy, but it is still true in general. So the Earth can trap the gas even though it is not a closed container.

In practice, gas in small container can be treated as uniformly distributed since the gravitational potential difference is small.

• Closer to the ground level, the gravitational pull is stronger, hence the density of gases will be greater. So, when we are considering the atmosphere as a whole, the gases aren't distributed uniformly and that's because of the differences in gas densities (at various heights). Is that correct? Commented Aug 10, 2013 at 12:10
• @AmalMurali Yes, the gas is not distributed uniformly for Earth atmosphere. It is easier to understand using pressure. As you go up mountain, the pressure decrease. The reason is the same Commented Aug 10, 2013 at 12:16
• @amalmurali Just in case it's not clear, note that the strength of Earth's gravity at an altitude of 100km is only slightly less than what it is at sea level, but the atmosphere at 100km is very thin. The air pressure at sea level is much higher because there is so much air on top of it, compressing it. Commented Apr 6, 2018 at 18:39

Of course gravity affects distribution.

That is why we have 'layers' of atmosphere surrounding the earth. The lower layers are very dense, and the density decreases as we go outwards, to zero in space.

When a limited amount of gas is released in a containter, it will fill up the space almost equally; the lower regions will be slightly denser (depends on how much gas is present and how tall the container is). If the container's height is comparable to the radius of the earth, then because of the mere weight of the gases on top, we'd have more pressure at the bottom - which is literally what's happened in the atmosphere! In the case of small containers - yes, even a ship could be considered small - the effect would be negligible, but in theory, the lower portions WOULD be denser, even by a really tiny amount.

Evem if you were to do it in space, the container in which you performed the experiment has mass, and subsequently its own gravitational field - and this would affect the distribution too.

However, if you completely remove gravity, then - yes, gas spreads out exactly evenly everwhere.

You've quoted from a kids' chemistry site. They obviously won't get into the depths of it - it's just basics, perhaps that's why they haven't mentioned it. See, they even mentioned that vapour and gases mean the same thing - although there is a difference. Vapour is definitely a gas and in the gaseous state, but not all gas is vapour!!! ;)

$P.S$: I finished + posted this answer more than 2 hours ago :/ Unfortunately my stupid internet connection conked off and it didn't post it until now, when I got connectivity again.

Well we know from experience that gas will eventually cluster together and form gravitational wells. Just looking at the sky shows proof of this (in the form of stars)*.

Yet that site is still a common description of gasses. How can this be? The difference stems from the model used.
The site talks about statistical/classical thermodynamics: It describes an ideal gas; a gas that to consist of hard particles which do not influence each other in any shape. So in this model there simply can't be any "gravitational" effect. Gravity is an effect where the molecules do react on each other, and as such the substance can no longer be described using the equations for an ideal gas

Now to describe this (and other) effects there are a lot of other models. However you should understand that for a lot of applications the classical thermodynamic laws are still valid (within error bounds).

*The exact effect of formation of stars is something non trivial though, simple Newtonian mechanics/gravity is too limited to describe this. This is an active field of study.

• Unfortunately, this doesn't answer my two questions. Commented Aug 10, 2013 at 12:12