I've come into this discussion a little late in the day, but...
By using air, providing you can get it to dissolve the gasses, you could get about 10 ppm of oxygen in the wort at say 10 deg C (I would have to look up the gas solubility tables, which I don't have to hand at present), but could in theory achieve about 30 ppm with pure oxygen instead (I have used oxygen to get to 18 + ppm, and know of one site that uses a mixture of air and oxygen with two separate injector systems to achieve 27 ppm).
However, all of this supposes you have very fine gas bubbles and approppriate back pressure, and suitable residence time to allow the gas to dissolve.
The key to dissolving the oxygen is to get extremely fine gas bubbles in the wort using a sinter, whether it is pure air, or pure oxygen.
If you want 1000 litres wort oxygenated to 10 ppm, then you need 10 grammes oxygen = 1.08 litres pure oxygen at 1 bar pressure (22.4 litres oxygen weighs about 32 g at 0 deg C and atmospheric pressure) . In other words, it sounds like your friends are nowwhere near dissolving all the oxygen, and are in fact wasting most of it (sorry but I only have the calcs in metric - use "Convert" or similar to get to US units)
By using air, providing you can get it to dissolve the gasses, you could get about 10 ppm of oxygen in the wort at say 10 deg C (I would have to look up the gas solubility tables, which I don't have to hand at present), but could in theory achieve about 30 ppm with pure oxygen instead (I have used oxygen to get to 18 + ppm, and know of one site that uses a mixture of air and oxygen with two separate injector systems to achieve 27 ppm).
However, all of this supposes you have very fine gas bubbles and approppriate back pressure, and suitable residence time to allow the gas to dissolve.
The key to dissolving the oxygen is to get extremely fine gas bubbles in the wort using a sinter, whether it is pure air, or pure oxygen.
If you want 1000 litres wort oxygenated to 10 ppm, then you need 10 grammes oxygen = 1.08 litres pure oxygen at 1 bar pressure (22.4 litres oxygen weighs about 32 g at 0 deg C and atmospheric pressure) . In other words, it sounds like your friends are nowwhere near dissolving all the oxygen, and are in fact wasting most of it (sorry but I only have the calcs in metric - use "Convert" or similar to get to US units)
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