The solubility of N2 in blood at 37 degreee Celcius and at a partial pressure of

Question

The solubility of N2 in blood at 37 degreee Celcius and at a partial pressure of 0.8atm is 5.6x10^-4 mol/L. A deep-sea diver breathes compressed air with the partial pressure of N2 equal to 4.5atm. Calculate the number of moles of N2 that are in the blood of the diver when breathing at this level in the deep-sea. Assume total volume of blood in the body is 5.0L. The solubility of N2 in blood at 37 degreee Celcius and at a partial pressure of 0.8atm is 5.6x10^-4 mol/L. A deep-sea diver breathes compressed air with the partial pressure of N2 equal to 4.5atm. Calculate the number of moles of N2 that are in the blood of the diver when breathing at this level in the deep-sea. Assume total volume of blood in the body is 5.0L.

Explanation / Answer

As per Henry's law

At constant temperature, the Solubility of a gas in a liquid is directly proportional to the pressure of that gas above it.The concentration can be calculated by the formula

Concentration = kHPgas

kH = 5.6 x 10-4 / 0.8 = 7 x 10-4 moles/L. atm (Both the parameters are given in the initial part)

Substitute this value in the latter case is Pgas = 4.5 atm

Concentration = kHPgas = 7 x 10-4 x 4.5 = 31.5 x 10-4 moles/L

Total number of moles of nitrogen molecule = concentration x volume in L = 31.5 x 10-4 moles/L x 5 L

= 157.5 moles of N2

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