Answer:
[tex]1.32\times 10^{-3} mol/L[/tex]is the solubility of nitrogen gas in a diver's blood.
Explanation:
Henry's law states that the amount of gas dissolved or molar solubility of gas is directly proportional to the partial pressure of the liquid.
To calculate the molar solubility, we use the equation given by Henry's law, which is:
[tex]C_{N_2}=K_H\times p_{liquid}[/tex]
where,
[tex]K_H[/tex] = Henry's constant = [tex]6.26 \times 10^{-4}mol/L.atm[/tex]
[tex]p_{N_2}[/tex] = partial pressure of nitrogen
[tex]p_{N_2}= P\times \chi_{N_2}[/tex] (Raoult's law)
[tex]=2.71 atm\times 0.78=2.1138 atm[/tex]
[tex]C_{N_2}=6.26 \times 10^{-4}mol/L.atm\times 2.1138 atm[/tex]
[tex]C_{N_2}=1.32\times 10^{-3} mol/L[/tex]
[tex]1.32\times 10^{-3} mol/L[/tex]is the solubility of nitrogen gas in a diver's blood.
