The concentration of n2 in blood at 37 °c (body temperature) and atmospheric pressure (partial pressure of n2 = 0.80 atm) is 0.00056 mol/l. a deep-sea diver breathes compressed air with the partial pressure of n2 equal to 4.0 atm. assume that the total volume of blood in the body is 5.0 l. calculate the mass and volume (at 37°c and atmospheric pressure (p(n2) = 0.80 atm) of n2 gas released as a diver surfaces.

volume  = 0.285 L

Explanation:

Henry constant is given as

Where C  is concentration

P is atmospheric pressure

when atmospheric pressure 4 atm

In 5 litere blood , moles of N_2

At surface moles  

Moles of N_2 release = 0.014 - 0.0028 = 0.0112

Mass of

T = 37 + 273 = 310 K

volume  = 0.285 L

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trachea, alveoli, lung capillaries, arteries