Question

At what partial pressure, oxygen will have a solubility of $0.006g{L}^{-1}$ in water at $293K$? Henry's law constant $\left(K_H\right)$ of $O_2$ in water at $303K$ is $46.82kbar$. (Assume the density of the solution to be the same as that of water).

Answer 1

No.of moles of water $=\frac{1000}{L8}=55.5mol$

no.of moles of oxygen $=\frac{0.006}{32}=0.0001875mole$

mole fraction of $O_2=\frac{18.75\times {10}^{-5}}{18.75\times {10}^{-5}+55.5}=3.37\times {10}^{-6}$

Partial pressure of $O_2=K_4\times x{O}_2$

$=46.82\times {10}^3\times 3.37\times {10}^{-6}$

$=0.157\times {10}^3$ Ans