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?

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  • 1 decade ago
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    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.

    Source(s): high school chemistry - you might have gotten an answer sooner had this question been posted under physics or chemistry, but here is your answer anyway!
  • ?
    Lv 4
    5 years ago

    Use the ideal gas equation PV=nRT to calculate how many moles of oxygen are in the tank. You know the volume, temperature and pressure. Calculate how many grams of O2 by multiplying the moles of O2 by the molecular weight of O2. I get 3.07 kg,

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