Question

The partial pressure of CO2 gas above the liquid in a carbonated drink is 0.51 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. Give your answer to 3 decimal places.

Answer 1

0.019 mol/L

Step-by-step explanation:

Given data

• Partial pressure of CO₂ above the liquid in a carbonated drink (P): 0.51 atm

• Henry's law constant for CO₂ (k): 3.7 × 10⁻² mol/L . atm

• Solubility of carbon dioxide in the drink (C): ?

According to Henry's law, the solubility of a gas in a liquid is proportional to its partial pressure.

C = k × P

C = (3.7 × 10⁻² mol/L . atm) × 0.51 atm

C = 0.019 mol/L

Answer 2

Answer: The molar solubility of carbon dioxide gas is 0.002 M

Step-by-step explanation:

Henry's law states that the amount of gas dissolved or molar solubility of gas is directly proportional to the partial pressure of the liquid.

To calculate the molar solubility, we use the equation given by Henry's law, which is:

`C_(CO_2)=K_H* p_(liquid)`

where,

`K_H` = Henry's constant =
`3.7* 10^(-2)mol/L.atm`

`p_(CO_2)` = partial pressure of carbonated drink = 0.51atm

Putting values in above equation, we get:

`C_(CO_2)=3.7* 10^(-2)mol/L.atm* 0.51atm\\\\C_(CO_2)=1.887* 10^(-2)mol/L=0.002M`

Hence, the molar solubility of carbon dioxide gas is 0.002 M