For divers going to great depths, the composition of the air in the tank must be modified. The ideal composition is to have approximately the same number of O2 molecules per unit volume as in surface air (to avoid oxygen poisoning), and to use helium instead of nitrogen for the remainder of the gas (to avoid nitrogen narcosis, which results from nitrogen dissolving in the bloodstream). Of the molecules in dry surface air, 78.0% are N2, 21.0% are 02, and 1.00% are Ar. (Assume that the density of seawater is 1025 kg/m and the temperature is 20.0°C.) Density of dry air at 20.0°C is 1.20 kg/m3. Molar mass of N2 is 14.007 g/mol, O2 is 15.999 g/mol, and Ar is 39.948 g/mol. (See Table B.7.)
For divers going to great depths, the composition of the air in the tank must be modified. The ideal composition is to have approximately the same number of O2 molecules per unit volume as in surface air (to avoid oxygen poisoning), and to use helium instead of nitrogen for the remainder of the gas (to avoid nitrogen narcosis, which results from nitrogen dissolving in the bloodstream). Of the molecules in dry surface air, 78.0% are N2, 21.0% are 02, and 1.00% are Ar. (Assume that the density of seawater is 1025 kg/m and the temperature is 20.0°C.) Density of dry air at 20.0°C is 1.20 kg/m3. Molar mass of N2 is 14.007 g/mol, O2 is 15.999 g/mol, and Ar is 39.948 g/mol. (See Table B.7.)
Chapter2: The Kinetic Theory Of Gases
Section: Chapter Questions
Problem 64P: Professional divas sometimes use heliox, consisting of 79% helium and 21% oxygen by mole. Suppose a...
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(a) How many O2 molecules per cubic meter are there in surface air at 20.0 degrees Celsius and 1.00 atm?
(b) For a diver going to a depth of 118 m, what percentage of the gas molecules in the tank should be O2 ?
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