Question

The partial pressure of CO2 gas above the liquid in a carbonated drink is 0.45 atm. Assuming that the Henry's law constant for CO2 in the drink is that same as that in water, 3.7 x 10-2 mol/L atm, calculate the solubility of carbon dioxide in this drink.

Answer 1

`M_(CO_2)=0.01665M`

Step-by-step explanation:

Hello,

In this case, the Henry's law allows us to relate the molar concentration and partial pressure of a solute (carbon dioxide) in a solution (solvent is water) by:

`M_(CO_2)=H_(CO_2)p_(CO_2)`

Whereas we introduce the Henry constant, therefore, we can easily compute the molar solubility by:

`M_(CO_2)=p_(CO_2)*H_(CO_2) =0.45atm*3.7x10^(-2)(M)/(atm)\\\\M_(CO_2)=0.01665M`

Regards.