Answer: The Henry's law constant for oxygen gas in water is [tex]1.702\times 10^{-5}g/mL.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] = solubility of oxygen gas = [tex]0.0043g/120.3mL[/tex]
[tex]p_{O_2[/tex] = partial pressure of oxygen gas = 2.1 atm
Putting values in above equation, we get:
[tex]0.0043g/120.3mL=K_H\times 2.1atm\\\\K_H=\frac{0.0043g}{120.3mL\times 2.1atm}=1.702\times 10^{-5}g/mL.atm[/tex]
Hence, the Henry's law constant for oxygen gas in water is [tex]1.702\times 10^{-5}g/mL.atm[/tex]
