Strangely, I enjoyed reading this thread. I am not sophisticated about th physics of tank filling, but I have filled thousands of tanks from a bank. Here is some observational data for the scients to incoprate in their continued explanation:
Thanks for the observations, Dennis. I'm going to comment on these points so that I can explain to myself why I think these things happen. I'm doing this in order to help me spot any errors in my conclusions, or possibly to let others spot those errors. I think I can explain all the observations consistently, and I think my comments wil also provide some answers to others who have urged me to track each step or stage of the filling process and apply the gas laws at each individual step or stage of the process.
1. The speed at which you fill a tank impacts the temperature of the receiving tank ( and the air in it). The faster you fill, the hotter it gets.
I think this happens because the faster you do it, the less time there is for the hot tank to cool. If we clamped both tanks together and wrapped the entire thing in insulation, I've calculated that the whole thing (both tanks and all the connecting valves, etc.) would all end up at room temp, no matter how quickly the transfer was made.
2. As the "hot" tank cools, the pressure reduces due to cooling of the contents, resulting in what was a 3000 PSI fill ending up being a 2400 psi fill ( more or less). The full cooling of the filled tank will take an hour or more on a hot summer day, even if in the shade.
I think this is just P/T=constant. As T drops, P also drops. It comes from the ideal gas law PV=nRT where volume is constant.
3. If you fill a tank at about 500 psi per minute or less, the heating is minimal, but it takes a long time to fill 50 tanks after the day's dive boat trip is done.
Same answer as for 1 above.
4. If you place the receiving tanks in cold water as you fill them, you can fill faster, as the heat dissipates quicker in the cold water ( just like the heat from a submerged diver's body).
This makes sense for the reason you give.
So, if anyone cares to assay this question, please explain the relationship between rte of fill and temperature of air in the recipient tank.
If you look at the gas laws - ideal gas law, Charles's law, Henry's law, etc. you'll see that none of them have any "time rate of change" factor. We can "calculate" the final temperature, pressure and volume without knowing the rate at which the changes were made.
However, all the fill operations we do aren't perfect the way those laws are perfect. They assume no energy gets lost, while in the real world, hot things cool off, so the longer we take to heat them up, the lower the final temperature.
---------- Post added February 24th, 2013 at 10:40 AM ----------
When you transfer gas from a bank of bottle to a empty scuba cylinder, the total change in energy is zero. the increase in temperature (total kinetic energy of the molecules) cancels out the drop in temperature of the gas bank. The bank is larger than the single cylinder so it is less noticable.
I agree with this.
---------- Post added February 24th, 2013 at 11:06 AM ----------
Both are correct. But the Joule Expansion is only theoretically possible. It does not reflect the reality of your question. That is, when filling one scuba tank from another, you do not meet the condition of thermal isolation necessary to produce the described results.
We agree that the real world isn't perfect, but no temperature change - Joule expansion was shown experimentally. If the receiving tank is thermally connected to the donor tank and the whole thing is wrapped in insulation we should have the same process.
I read several descriptions of the Joule expansion experiments. In one, they put the receiving tank inside the donor tank, then opened the connecting valve. The gas arriving in the inner receiving tank got hot. The gas remaining in the outer donor tank cooled off. The whole thing was wrapped in insulation to prevent any heat getting to the cold outer tank. IOW, the energy added or removed from the system was zero. When the gas of the inside tank stopped cooling and the gas of the outside tank stopped being heated by the inside tank, the temperature of both tanks was the same and that temp was unchanged from the original temperature.
That tells me that the fundamentals of filling a tank from another tank are the same as in Joule expansion/free expansion.
Sure, a compressor adds a thermal source
I was writing quickly and didn't mean to imply that a compressor adds any heat energy. (In the real world it does, but that's not where the heat comes from) Energy is work plus heat energy. The compressor is doing "work" - applying a force to the gas and moving it a distance to force it into the tank.
We can assume that all the energy added is in the form of work - not heat. Then we just need to solve PV=nRT to get the new temperature and pressure knowing the change in volume - the starting volume of air (80 cubic feet) and the final volume (the tank's true volume). To do that, we need to solve for two unknowns, P and T, but the ideal gas law is only one equation. The other equation I referred to in my first post - (P times V to the power gamma) is constant, where gamma is about 1.4 for air. There's no heat being added, just mechanical work energy, when the donor tank is being filled. I put in those two equations in my very first post to try to draw out the expertise of someone who had looked at the "fill from a higher pressure tank" process from a similar science/physics/math perspective.
but even with bank tanks, the event is not thermally isolated
I agree it's not normally thermally isolated, but the whole effect doesn't go away as we wrap insulation around everything. If anything, the effect becomes more pronounced.
and adiabatic heating and cooling occur and the gas molecules take up and give of energy as the pressures change during the fill process.
We agree that different parcels of gas go through different PVT changes during the process, but as long as we know that no heat is added and no work is done on the system, then we know that the system energy is unchanged. As long as energy is unchanged, all we need are the final pressures and volumes to determine the final temperatures.