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The molecules which make up the walls of the container are also undergoing random thermal motion.If you put a hot gas into a cold container, the gas molecules will on average lose energy during their ...

Everything you've said is correct, which is why the conclusion is: there is no fundamental difference! Under the modern classification, they're just the same fluid phase of matter.For example, ...

The described measurement would allow you to construct the Radial Distribution Function, the probability of finding another particle a distance r from a reference particle usually given as g(r), which ...

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The law $PV = n RT$ gives the pressure $P$ of $n$ moles of ideal gas in volume $V$. Meanwhile, the law $\Pi V = n R T$ describes the osmotic pressure $\Pi$ due to $n$ moles of solute in volume $V$. ...

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The mean-free path of a nitrogen molecule in air at STP is about 60 nm, so the molecules may travel quite quickly, but they do not go very far before the run into another molecule and get stopped.

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I notice that online definitions of this experimental law always say, molecules or atoms.The problem with just calling them all "molecules" and being done with it is some are uncomfortable with using ...

You don't need a container, you need a force. Walls of a container can provide a force, but gravity also works. The escape velocity of the earth at sea level is about 11.2 km/s. The mean velocity of ...

In a gas the molecules move separately. In a liquid they cling together due to van der Waals forces which are strong enough that the vibrating molecules do not completely separate.

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The question may be aiming to expand one's scope beyond what's considered in introductory textbooks. This is the essence of scientific research.The heat capacity $C_X$ at a condition of constant $X$ ...

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It is an interesting question with an answer, but it is not simple for at least three important reasons. The first one is that, to provide a precise answer, one should know quit well the progresses ...

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No you cannot. we can show that (via conservation of kinetic energy and momentum) the speed of the particle before and after collision is the same.Only in the center of mass of two elastically ...

It might be worth pointing out that at molecular level, perfectly elastic collisions can happen. Take for example two protons. When they are stationary & at distance $r$ apart, their kinetic ...

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I know that inelastic collision(e=0) of gas molecules does not make sense, but I wonder, if somehow hypothetically gas molecules made inelastic collision with the container in which it is filled and ...

I thought of this question while waiting for a warm room to cool downafter opening a window.A warm room is not just composed of warm air. The whole building has a huge thermal mass (basically, the ...

I remember reading a FlErF's complaint: if the Earth is a ball, then space would vacuum the atmosphere away.Believe me: it's trying.An order magnitude estimate proceeds like this:We approximate the ...

Thermodynamic equilibriumEnergy is conserved in collisions. Collisions between the atoms/molecules lead to exchange of energy between these atoms/molecules, whereas collisions with the walls of the ...

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There is no pressure gradient.The way to see this is to find a static solution to the equation of fluid dynamics. The Euler equation is$$\partial_t\vec{v}+(\vec{v}\cdot\vec{\nabla})\vec{v} = -\frac{...

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The reason is that $f(E)$ is not a probability density function (this is a misinterpretation of some sloppy sources), but it’s the mean occupation number of a state, that is, it’s the mean number of ...

There are various conditions which might apply while a gas expands.adiabatic (isentropic) expansion. Gas does work on its surroundings (pushing on the boundary as the boundary moves) so loses energy....

The macroscopic kinetic energy of a system of particles is the kinetic energy due to the velocity of the center of mass of the collection of particles with respect to an external frame of reference....

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Semoi's answer is good. But since you say I would prefer an intuitive explanation rather than a mathematical oneto express it more simply, and without formulae, the Maxwell distribution is the chi ...

There has actually been a fair amount of activity in this area recently, see, for example, this set of lecture notes.I would argue that the answer to your question is, "yes", if properly ...

Both pressure and temperature can be thought of as forms of kinetic energy density, but they are divided over different quantities. Pressure is proportional to kinetic energy per unit volume, while ...

Even if initial speed of all the particles was same, the molecular collisions will disrupt this uniformity. I want to show this happens based on a diagram (on the left) from one of Maxwell's papers. ...

Imagine that you're in a large room - say, 50 m x 50 m - which is so filled with people that on average you only travel about 1 meter before colliding with somebody else. Everyone on the left side ...

In addition to what @mike stone said, keep in mind that heat transfer from the higher temperature side, say left side of the container, to the lower temperature side, say right side of the container ...

If uniform distribution is promised as equilibrium, it means the zero external force $\mathbf{F}$, which means that the $\nabla_\mathbf{p}f$ can have any value. without violating the equation.As an ...

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There are several mechanisms which can serve to increase the kinetic energy of a system. Any of these might be ways in which heat / energy is added to the kinetic rather than potential energy. I'll ...

A gas need not have a "container" in the sense of being enclosed inside some material to have pressure. The particles of a gas need to have a minimum mean kinetic energy for the substance to ...

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What is the viscosity of Sun surface?By "solar surface" I am going to assume you mean the photosphere. In that case, then the question is whether you are asking about dynamic ($\mu$) or kinematic ($\...