# What is the pressure at a random point inside container of an ideal gas?

In most textbooks and thermodynamic lectures, the pressure is defined as the force on the walls of containers due to the incassecant beating of gas molecules divided by the area of the wall. Now, suppose I take a random point inside the container, what would be it's pressure at equilibrium and also non equilibrium conditions?

I am confused on the point whether we should have a wall or not to define pressure like is pressure a quantity defined 'over' the boundary of the container and undefined inside and outside? This seemed strange, to resolve, I thought of taking some random surfaces inside the container (say maybe a imaginary sphere) and then computing the pressure.

If the gas is in equilibrium,

$$P \overline{V} = RT$$

and, if we calculate temperature from the temp of gas (all points have same because equilibrium) then we find pressure same for all points inside a gas. However this still is weird because how can you talk of 'pressure' without having a physical membrane which is being hit upon.