Answer: The Henry's constant for oxygen gas is [tex]3.81\times 10^{-2}g/L.atm[/tex]
Explanation:
To calculate the molar solubility, we use the equation given by Henry's law, which is:
[tex]C_{O_2}=K_H\times p_{O_2}[/tex]
where,
[tex]K_H[/tex] = Henry's constant = ?
[tex]C_{O_2}[/tex] = molar solubility of oxygen gas = [tex]0.590g/L[/tex]
[tex]p_{O_2}[/tex] = partial pressure of oxygen gas = 15.5 atm
Putting values in above equation, we get:
[tex]0.590g/L=K_H\times 15.5atm\\\\K_H=\frac{0.590g/L}{15.5atm}=3.81\times 10^{-2}g/L.atm[/tex]
Hence, the Henry's constant for oxygen gas is [tex]3.81\times 10^{-2}g/L.atm[/tex]
