Actually, I didn't observe that. I learned it later. I did observe the heating, but didn't notice whether it got hotter or colder than air.Close oh so close. . . so you've observed that filling a tank with O2 warms it more than filling it with air.
I agree, there is a difference. It has to do with real world differences between ideal gases and real gases. However, air, and oxygen both heat up for the same basic reason, even though the temperature change is different.Ergo, something about air is different than pure O2.
You're thinking of the fact that He and H both have a slightly negative Joule-Thomson coefficient at common pressures, while air has a slightly positive J-T coefficient. Ideal gases have a zero J-T coefficient. What this means is that at "constant enthalpy," air will heat slightly when expanded in a Joule-Thomson "free expansion" process, an ideal gas will not change temperature and He and H will slightly cool as they expand in the constant enthalpy process.If you were to observe a tank being filled with He, you'd observe slight cooling.
I know "enthalpy" is a pretty geeky term, but it just means that the internal energy of the gas in the system is unchanged. What this means is that if we filled the receiving tank with air from another higher pressure donor tank (as we've been discussing) and don't add or subtract any energy) the tank gets slightly hotter instead of remaining at constant temperature as described for the Joule expansion process, while He gets slightly cooler when it expands.
These are second order effects that deviate from the ideal gas law. By that I mean that air gets slightly cooler when it is compressed than an ideal gas, but that doesn't mean that compressing air with an air compressor will make the air colder. When you use a compressor to compress air, you are not engaged in a constant enthalpy process. You are increasing the "internal energy" of the gas and the J-T coefficient effect is just slight modification to the heating that occurs. The air gets slightly cooler than expected when it undergoes that compression even though the net effect is that the air gets hotter.
We can account for them if we need to, but it won't have a major effect.But wait ! This isn't accounted for by the Ideal Gas Law (or any of the equations you reference which are based on Ideal Gas(s) )
It's not. It's just that the ideal gas is pretty close to the non-ideal gas and using the ideal gas laws will give the basic answers. Charles's Law still works pretty well.Simple. Gas(s) are not ideal. Why is this such a problem for you?
I agree that He will cool. The He fill process is always a fill from an existing tank at higher pressure, which is a nearly constant enthalpy Joule expansion process.Since you're getting twisted around by the equations (you've stated this many time), take a trip to your local technical LDS and ask to watch them fill a tank with He and the same pressure of O2. Measure the temperature change and get back to us. Right now you're just indulging in mental masturbation and counting (and re-counting) how many Angels are dancing on that pin.
Do you know what would happen if the room was filled with He and a compressor was used to take low pressure He at room temp and force it into the tank? That would be a constant entropy process, not constant enthalpy. The internal energy of the He would increase. The He would be heated and the amount of heating would be partly due to the increased internal energy (the same reason air is heated when compressed by a compressor) plus some additional heating due to the negative J-T coefficient of He. The second order effect is that He would get slightly hotter than expected, just as air gets slightly colder than expected when compressed by a compressor.
It's not angels on the head of a pin. It's physics.
---------- Post added February 24th, 2013 at 03:22 PM ----------
At least we agree about this.Are you ****ing kidding me? Of course the gas started at a higher pressure! That cannot be ignored. Why? Because there's no other way to get it out of the donor tank and into the receiving tank other than to have a pressure gradient sufficient to overcome the pressure inside the receiving tank.
Is this a trick questionPlease answer the two questions below:
After the tanks equalize, you close the valves and remove the fill whip. You put a reg and a BCD on the tank, open the valve, strap it to your back, and jump in the water. With the reg in your mouth, you attempt to draw a breath from the tank.
1.) What happens?
2.) Why?
1.) The gas passes through the regulator and expands into your lungs.
2.) The pressure differential and regulator act to ensure that the pressure in your lungs and the output of the regulator equalize.
I'm not sure where you're going with this.
---------- Post added February 24th, 2013 at 03:47 PM ----------
I noticed you didn't answer mine, which scarcely seems fair.Well, I did ask for a one word answer.....
Anyhow, forget the freakin equations. So, you do agree that when gas gets compressed it warms up.
Next question, one word answer, yes or no. Do you accept the fact that the gas in the recipient tank is getting compressed?
If you tell me the starting temperature, pressure and volume of the gas you are talking about, I'll tell you whether the gas is getting compressed.
What case are we talking about? There is no gas in the recipient tank if it's evacuated, so I answer NO - it's not getting compressed. That's a simpler case to deal with and would answer my question if anyone could explain .
If the recipient tank was not evacuated, and had some air at room temperature, then I answer YES. The air that started in there is getting compressed. That gas gets hotter. That heat is not enough to explain the amount of heat produced, but it does have a small effect. There is also a small effect from the non-zero J-T coefficient of air.
Why don't you answer these questions for me.It really is as simple as that. Consider this one of those glorious times in the universe when there's a super-easy-peezy answer.
1) Do you agree it took energy to compress the gas into the donor tank?
2) Do you agree that we could get some of that energy back by putting a pneumatic motor/generator in the whip line between the tanks and driving the generator by the pressure differential during the fill?
3) Do you agree that the recipient tank and donor tank would equalize pressure regardless of whether we put a pneumatic motor/generator in the whip line?
4) What happened to all the energy we could have extracted from the pneumatic motor/generator if we didn't put the pneumatic motor/generator in the whip line?
Good idea.Now put down the equations and go outside, have some fun!
Particular thanks to JohnN. His J-T coefficient comments took me the most effort to figure out.
RJP's and your thoughts on compressing the preexisting air in the tank were also good, but didn't deal with the evacuated tank problem. I could show mathematically that the heating of the preexisting air isn't enough, but that should be apparent from the evacuated tank problem.
I forget who raised the possibility of heat leaking into the system at the cold valve, but thanks to him, Until I understood Joule expansion (free expansion) and the difference between constant entropy and constant enthalpy expansion, I thought that was the answer.
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