Answer: The pressure of carbon dioxide needed is 2.94 atm
Explanation:
To calculate the partial pressure of carbon dioxide, 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]3.4\times 10^{-2}mol/L.atm[/tex]
[tex]C_{CO_2}[/tex] = molar solubility of carbon dioxide gas = [tex]0.10mol/L[/tex]
[tex]p_{CO_2}[/tex] = pressure of carbon dioxide = ?
Putting values in above equation, we get:
[tex]0.10mol/L=3.4\times 10^{-2}mol/L.atm\times p_{CO_2}\\\\p_{CO_2}=\frac{0.10mol/L}{3.4\times 10^{-2}mol/L.atm}=2.94atm[/tex]
Hence, the pressure of carbon dioxide needed is 2.94 atm
