Pressure can be explained at microscopic level for a gas with kinetic theory of gases. From that the pressure $p$ is linked to the velocity of molecules (and it is caused by the high amount of collisions in the gas).
$$p=\frac{m N_a}{V} \frac{\bar{v}^2}{3}$$
Where $m$ is the mass of a molecule, $N_a$ Avogadro's number, $V$ volume, $\bar{v}^2$ the quadratic average velocity of molecules.
Nevertheless I did not find a similar microscopic interpretation in the case of liquids. In that case molecules are not as free as in a gas, so it looks like pressure is not linked to the higher or lower velocity of molecules. So what is responsible for liquid pressure, at a microscopic level?
Is there a quite simple microscopic description for pressure in liquids, as there is in the kinetic theory of gases?
Best Answer
Unlike a gas a liquid has a finite volume at zero pressure i.e. a liquid floating in vacuum would not expand beyond a certain volume. This volume is determined by the interatomic/intermolecular forces in the liquid.
If you look at the potential energy between two liquid molecules as a function of intermolecular distance $r$ it will be something like:
(picture from here)
And the zero pressure volume will be the one where the intermolecular distances are at the minimum of the potential energy. This will be your zero pressure volume. If you compress the liquid you push the molecules up the higher potential energy curve towards smaller $r$, and that takes work, i.e. a force, which is why the compressed liquid has a pressure.
There is some effect of molecular motion, and indeed that's why liquids (usually) expand when you heat them. The potential well is not symmetric, so as you add thermal energy the mean intermolecular distance moves to larger $r$. However the main mechanism for sustaining a pressure is the intermolecular potential.