5.5 × 10⁻⁴ mol/L is the molarity of N₂ in blood at 1.00 atm.
The gas law that states that if the constant is in terms of solubility or pressure.
It is expressed as
Solubility = Henry constant × Partial Pressure
Air contains 78% N₂ by volume.
Mole fraction of N₂ = [tex]\frac{78}{100}[/tex]
= 0.78
Henry constant for N₂ is 7.0 × 10⁻⁴ mol/L
Pressure is given 1.00 atm
Mole fraction = 0.78
Now find the partial pressure,
Partial Pressure of N₂ = Mole Fraction × Total Pressure
= 0.78 × 1 atm
= 0.78 atm
Now put the values in above equation to find the solubility
Solubility = Henry constant × Partial Pressure
= 7.0 × 10⁻⁴ mol/L.atm × 0.78 atm
= 5.5 × 10⁻⁴ mol/L
Thus from the above conclusion we can say that 5.5 × 10⁻⁴ mol/L is the molarity of N₂ in blood at 1.00 atm.
Learn more about the Henry Law here: https://brainly.com/question/23204201
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