I've been trying to wrap my mind around this for the last couple of days to no avail. I suspect that much of my confusion comes from the fact that I have not yet taken a class specifically focused on thermodynamics, so my current perception of this likely holds a number of fundamental misunderstandings.
My question, essentially, is what exactly the relationship between temperature and pressure is in a massive volume of a fluid. To clarify (I hope) the aim of my inquiry, I began thinking about this from the perspective of my rudimentary understanding of the temp/pressure relationship in ideal gasses. From this perspective, temperature and pressure seem to be two sides of the same coin - two (equivalent?) measures of the energy in the system available to do work on its surroundings, because both are determined by the kinetic energy transferred over the sum of particle collisions being observed.
So, in a massive volume of fluid where pressure increases greatly with depth, could that fluid come to state of thermal equilibrium? If it can, how do we explain why the the temperature near the surface at relatively low pressures is the same as the temperature at larger depths and pressures within the same volume? If the pressure is greater at depth, that must mean that there are more particle collisions over a unit time than at low pressures (more energy transferred to an observer at these depths), and would this not also imply a higher temperature???
I hope the aim of my question here is discernible