What is the solubility of CO₂, in molarity units, in 1.0 L of water when the partial pressure of CO₂ is 1.8 atm?

Question

The Henry's law constant at 25 °C for CO₂ in water is 0.035 M/atm. What is the solubility of CO₂, in molarity units, in 1.0 L of water when the partial pressure of CO₂ is 1.8 atm?

Answer 1

Henry's law states that the solubility of a gas is directly proportional to the vapor pressure of that gas above the liquid. The proportionality constant is referred to as Henry's constant.

C = P/k

C = concentration (solubility)

k = Henry's constant = 29 Latm/mol (I looked it up)

P = partial pressure = 1.8 atm

C = 1.8 atm / 29 Latm/mol

C = 0.062 moles/liter = 0.062 M