Answer: The Henry's constant for carbon dioxide is [tex]3.38\times 10^{-2}mol/L.atm[/tex]
Explanation:
To calculate the molar solubility, we use the equation given by Henry's law, which is:
[tex]C_{CO_2}=K_H\times p_{CO_2}[/tex]
where,
[tex]K_H[/tex] = Henry's constant = ?
[tex]C_{CO_2}[/tex] = molar solubility of carbon dioxide gas = [tex]2.2\times 10^{-1}mol/L[/tex]
[tex]p_{CO_2}[/tex] = partial pressure of carbon dioxide gas = 6.5 atm
Putting values in above equation, we get:
[tex]2.2\times 10^{-1}mol/L=K_H\times 6.5atm\\\\K_H=\frac{2.2\times 10^{-1}mol/L}{6.5atm}=3.38\times 10^{-2}mol/L.atm[/tex]
Hence, the Henry's constant for carbon dioxide is [tex]3.38\times 10^{-2}mol/L.atm[/tex]
