oxygen
Roughly 3.123 liters (at the same pressure). Nitrogen is 78.08% of dry air by volume. 3.123 liters of nitrogen at STP is about 0.14 moles, or just under 2 grams.
Two liters divided by 3.2 ATM => 0.625 liters / 1 ATM >> ought to do it.
4.7 times the ambient air pressure which is ? Need more data...
390 liters
2 volumes of ammonia gas.
Nitrogen comprises 78% of the composition of air. Therefore the nitrogen would be 78% of the 2L:2000mL x 0.78 = 1560mL1560mL = 1.56L
Assuming the medium is fresh water at room temperature and atmospheric pressure, then the density is 1 gram per one milliliter 28000 grams = 28000/1 = 28000 milliliter = 28 liters (as 1 liter = 1000 milliliter)
1000 liters
According to metal-wear, one liter of LN2 will make 22.8 standard cubic feet (scf) of gas. 1 scf equals approximately 1 FTS, the exact conversion depends on the ambient temperature and pressure. So 1000 FTS / 22.8 scf = 43.9 liters of liquid nitrogen.
One cubic meter always has 1000 liters, no matter what is inside. On the other hand, 6 bars is approximately 6 times the normal atmospheric pressure, so - according to the ideal gas law - the cubic meter of compressed air would be equivalent to 6 cubic meters of "normal" air.
0.9 gm
To work this out there are two possible methods, the first uses knowledge about densities: At it boiling point, Liquid Nitrogen has a density of 807.0 grams per liter At Standard Temperature and Pressure, Nitrogen Gas has a density of 1.251 grams per liter Thus:- 25 liters of Liquid Nitrogen will weigh 25*807 = 20175 grams At STP 20175 grams of Nitrogen Gas will occupy 20175/1.251 = 16127.1 liters. The second method is to use the published expansion ratio for Liquid Nitrogen: Liquid Nitrogen has a liquid-to-gas expansion ratio of 1:694 at 20°C (68 °F) Thus:- 25*694=17350 liters. You will see the numbers are similar but slightly different, of the two I would be more confident in the density calculation method result. Although I suspect most people would use the expansion ratio method.