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a 5000 cc scuba tank filled to 50 atm pressure at 30 degrees C with a standard air mix. Using daltons law of p?
a 5000 cc scuba tank filled to 50 atm pressure at 30 degrees C with a standard air mix. Using daltons law of partial pressure, how many moles of oxygen are in the tank?
First let’s convert the volume of air to STP, which is a pressure of 1 atm. and temperature
of 0°C or 273°K. Our given pressure is 50 atm. and 30°C or 303°K, and the volume of the
tank is 5000 cc, or 5.0 liters. Ordinary air contains about 21% oxygen and 78 nitrogen,
so the partial pressure in the tank is 50 times 0.21, or 10.5 atmospheres that is oxygen.
So at STP the volume of just the oxygen would be 5 liters * 10.5 * 273/303 = 47.3 liters.
At STP one mole of any gas occupies a volume of 22.414 liters,
so we have 47.3/22.414, or 2.11 moles of oxygen in the tank.
Hope this answers your question.
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