Answered

Arterial blood contains about 0.25 g of oxygen per liter at 37°C and standard atmospheric pressure. Under these conditions, the Henry's law constant is kH = 3.7 × 10^–2 mol/(L • atm), and the mole fraction of O2 in the atmosphere is 0.209

Calculate the solubility (in M) of O2 in the blood of a scuba diver at a depth of 100 feet, where Patm = ~3 atm

_______ M

Sagot :

The solubility (in M) of O2 in the blood of a scuba diver at a depth of 100 feet is 2.32 × 10^-3 mol.

How to calculate the solubility?

It should be noted that the partial pressure of oxygen will be:

= Mole fraction × Total pressure

= 0.209 × 3

= 0.627

According to Henry's law, the solubility will be:

= 3.7 × 10^-2 × 0.627

= 2.32 × 10^-3 mol

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